OCR GCSE 9-1 Gateway Science/Chemistry QUIZ on Topic C3 "CHEMICAL REACTIONS" (FT)

Which four quantities a, b, c and d are required to balance the equation ...
aCH_4(g) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-1]
1. 1 2 1 2
2. 1 1 1 2
3. 1 2 2 1
4. 1 1 1 1
Which four quantities a, b, c and d are required to balance the equation ...
aC₂H_6(g) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-2]
1. 1 2 1 3
2. 2 7 4 6
3. 2 4 4 6
4. 1 7 2 3
Which four quantities a, b, c and d are required to balance the equation ...
aC₃H_8(g) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-3]
1. 1 3 3 4
2. 2 10 4 6
3. 1 5 3 4
4. 2 5 2 3
Which four quantities a, b, c and d are required to balance the equation ...
aC₄H_10(g) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-4]
1. 1 13 8 4
2. 2 7 4 10
3. 1 5 3 4
4. 2 13 8 10
Which four quantities a, b, c and d are required to balance the equation ...
aC₅H_12(l) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-5]
1. 1 8 5 6
2. 1 4 4 6
3. 2 4 5 12
4. 2 8 10 12
Which four quantities a, b, c and d are required to balance the equation ...
aC₆H_14(g) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-6]
1. 2 9 6 14
2. 2 19 12 14
3. 1 9 6 7
4. 1 10 12 7
Which four quantities a, b, c and d are required to balance the equation ...
aC₇H_16(l) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-7]
1. 1 5 7 8
2. 2 12 14 16
3. 1 11 7 8
4. 2 11 14 16
Which four quantities a, b, c and d are required to balance the equation ...
aC₈H_18(g) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-8]
1. 1 13 8 18
2. 1 13 8 9
3. 2 13 16 18
4. 2 25 16 18
Which four quantities a, b, c and d are required to balance the equation ...
aC₂H_4(g) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-9]
1. 1 3 2 2
2. 1 2 2 2
3. 2 3 4 4
4. 2 6 4 4
Which four quantities a, b, c and d are required to balance the equation ...
aC₃H_6(g) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-10]
1. 2 5 6 6
2. 2 9 6 6
3. 1 5 3 3
4. 1 9 3 3
Which four quantities a, b, c and d are required to balance the equation ...
aC₄H_8(g) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-11]
1. 2 12 8 8
2. 2 6 8 8
3. 1 6 4 4
4. 1 3 4 4
Which four quantities a, b, c and d are required to balance the equation ...
aC₇H_8(g) + bO_2(g) ==> cCO_2(g) + dH₂O_(l) ?[eq-12]
1. 2 9 4 8
2. 2 10 14 8
3. 1 5 7 4
4. 1 9 7 4
Which three quantities a, b and c are required to balance the equation ...
aFe_(s) + bO_2(g) ==> cFe₃O_4(s) ? [eq-13]
1. 3 2 1
2. 3 4 1
3. 6 4 2
4. 6 2 2
Which three quantities a, b and c are required to balance the equation ...
aLi_(s) + bO_2(g) ==> cLi₂O_(s) ? [eq-14]
1. 2 1 2
2. 4 1 2
3. 4 2 1
4. 2 2 1
Which three quantities a, b and c are required to balance the equation ...
aAl_(s) + bO_2(g) ==> cAl₂O_3(s) ? [eq-15]
1. 1 3 2
2. 4 6 4
3. 4 3 2
4. 2 3 2
Which three quantities a, b and c are required to balance the equation ...
aMg_(s) + bO_2(g) ==> cMgO_(s) ? [eq-16]
1. 1 1 2
2. 4 2 2
3. 2 1 1
4. 2 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aZn_(s) + bHCl_(aq) ==> cZnCl_2(aq) + dH_2(g) ? [eq-17]
1. 1 2 1 1
2. 2 2 2 1
3. 2 1 1 2
4. 1 1 2 2
Which four quantities a, b, c and d are required to balance the equation ...
aFe_(s) + bH₂SO_4(aq) ==> cFeSO_4(aq) + dH_2(g) ? [eq-18]
1. 1 1 1 2
2. 1 1 1 1
3. 2 2 2 1
4. 2 1 2 2
Which four quantities a, b, c and d are required to balance the equation ...
aAl_(s) + bHCl_(aq) ==> cAlCl_3(aq) + dH_2(g) ? [eq-19]
1. 1 6 3 2
2. 2 3 2 3
3. 2 6 2 3
4. 1 3 3 2
Which four quantities a, b, c and d are required to balance the equation ...
aAl_(s) + bH₂SO_4(aq) ==> cAl₂(SO₄)_3(aq) + dH_2(g) ? [eq-20]
1. 1 3 1 3
2. 2 3 2 3
3. 1 2 2 2
4. 2 3 1 3
Which four quantities a, b, c and d are required to balance the equation ...
aNa_(s) + bH₂O_(l) ==> cNaOH_(aq) + dH_2(g) ? [eq-21]
1. 2 2 2 1
2. 2 1 2 1
3. 1 2 1 2
4. 1 1 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aCa_(s) + bH₂O_(l) ==> cCa(OH)_2(aq) + dH_2(g) ? [eq-22]
1. 2 2 2 1
2. 1 2 1 1
3. 1 2 1 2
4. 2 1 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aFe_(s) + bH₂O_(g) ==> cFe₃O_4(s) + dH_2(g) ? [eq-23]
1. 3 4 1 2
2. 2 3 1 4
3. 3 4 1 4
4. 2 3 2 2
Which four quantities a, b, c and d are required to balance the equation ...
aAl_(s) + bH₂O_(g) ==> cAl₂O_3(s) + dH_2(g) ? [eq-24]
1. 3 4 1 6
2. 1 3 1 3
3. 2 4 2 6
4. 2 3 1 3
Which four quantities a, b, c and d are required to balance the equation ...
aMg_(s) + bCuSO_4(aq) ==> cMgSO_4(aq) + dCu_(s) ? [eq-25]
1. 1 1 1 1
2. 2 1 2 2
3. 1 2 1 2
4. 2 2 2 1
Which four quantities a, b, c and d are required to balance the equation ...
aCu_(s) + bAgNO_3(aq) ==> cCu(NO₃)_2(aq) + dAg_(s) ? [eq-26]
1. 1 1 2 1
2. 1 2 1 2
3. 2 2 1 2
4. 2 2 2 1
Which four quantities a, b, c and d are required to balance the equation ...
aZn_(s) + bFe₂(SO₄)_3(aq) ==> cZnSO_4(aq) + dFe_(s) ? [eq-27]
1. 3 2 6 2
2. 3 1 3 3
3. 3 1 3 2
4. 2 2 6 3
Which four quantities a, b, c and d are required to balance the equation ...
aAl_(s) + bFe₂O_3(s)) ==> cAl₂O_3(s) + dFe_(s) ? [eq-28]
1. 1 2 2 1
2. 3 1 1 3
3. 2 3 2 3
4. 2 1 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aCl_2(aq) + bKBr_(aq) ==> cKCl_(aq) + dBr_2(aq) ? [eq-29]
1. 1 2 2 1
2. 2 1 1 1
3. 1 1 2 2
4. 2 2 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aBr_2(aq) + bNaI_(aq) ==> cNaBr_(aq) + dI_2(aq) ? [eq-30]
1. 1 2 1 2
2. 1 2 2 1
3. 1 1 2 2
4. 2 2 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aCl_2(aq) + bCaI_2(aq) ==> cCaCl_2(aq) + dI_2(s) ? [eq-31]
1. 2 1 2 1
2. 1 2 2 2
3. 1 1 1 1
4. 2 2 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aAlBr_3(aq) + bCl_2(aq) ==> cAlCl_3(aq) + dBr_2(s) ? [eq-32]
1. 1 3 2 2
2. 1 3 1 3
3. 3 2 2 2
4. 2 3 2 3
Which five quantities a, b, c, d and e are required to balance the equation ...
aCaCO_3(s) + bHCl_(aq) ==> cCaCl_2(aq) + dH₂O_(l) + eCO_2(g) ? [eq-33]
1. 1 2 1 1 1
2. 2 2 1 2 1
3. 1 1 1 1 1
4. 2 1 2 2 2
Which five quantities a, b, c, d and e are required to balance the equation ...
aNa₂CO_3(s) + bHCl_(aq) ==> cNaCl_(aq) + dH₂O_(l) + eCO_2(g) ? [eq-34]
1. 1 4 4 2 2
2. 1 2 2 1 1
3. 2 2 4 2 2
4. 2 2 2 1 1
Which five quantities a, b, c, d and e are required to balance the equation ...
aTl₂(CO₃)_3(s) + bHCl_(aq) ==> cTlCl_3(aq) + dH₂O_(l) + eCO_2(g) ? [eq-35]
1. 2 6 4 3 6
2. 1 3 2 6 2
3. 1 6 2 3 3
4. 2 3 4 3 6
Which five quantities a, b, c, d and e are required to balance the equation ...
aTl₂(CO₃)_3(s) + bH₂SO_4(aq) ==> cTl₂(SO₄)_3(aq) + dH₂O_(l) + eCO_2(g) ? [eq-36]
1. 2 6 4 3 6
2. 1 3 2 6 6
3. 1 6 2 6 3
4. 1 3 1 3 3
Which three quantities a, b and c are required to balance the equation ...
aNa_(s) + bCl_2(g) ==> cNaCl_(s) ? [eq-37]
1. 2 1 2
2. 1 1 1
3. 1 2 1
4. 2 1 1
Which three quantities a, b and c are required to balance the equation ...
aAl_(s) + bCl_2(g) ==> cAlCl_3(s) ? [eq-38]
1. 1 3 1
2. 2 3 2
3. 2 2 3
4. 1 3 2
Which three quantities a, b and c are required to balance the equation ...
aCa_(s) + bCl_2(g) ==> cCaCl_2(s) ? [eq-39]
1. 1 2 1
2. 1 1 2
3. 1 1 1
4. 2 2 1
Which three quantities a, b and c are required to balance the equation ...
aP_(s) + bCl_2(g) ==> cPCl_5(s) ? [eq-40]
1. 1 5 1
2. 1 5 2
3. 2 5 4
4. 2 5 2
Which four quantities a, b, c and d are required to balance the equation ...
aFe₂O_3(s) + bCO_(g) ==> cFe_(l) + dCO_2(g) ? eq-41]
1. 1 3 2 3
2. 1 6 2 6
3. 2 6 4 3
4. 2 3 4 6
Which four quantities a, b, c and d are required to balance the equation ...
aCuO_(s) + bH_2(g) ==> cCu_(l) + dH₂O_(g) ? [eq-42]
1. 2 1 1 1
2. 1 1 1 1
3. 1 2 2 1
4. 2 1 2 1
Which four quantities a, b, c and d are required to balance the equation ...
aCuO_(s) + bC_(s) ==> cCu_(s) + dCO_2(g) ? [eq-43]
1. 1 2 1 2
2. 2 2 2 1
3. 2 1 2 1
4. 1 1 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aFe₃O_4(s) + bC_(s) ==> cFe_(l) + dCO_2(g) ? [eq-44]
1. 2 1 3 2
2. 1 3 2 1
3. 2 1 2 1
4. 1 2 3 2
Which four quantities a, b, c and d are required to balance the equation ...
aNaOH_(aq) + bHCl_(aq) ==> cNaCl_(aq) + dH₂O_(l) ? [eq-45]
1. 1 1 1 1
2. 1 2 2 1
3. 2 1 1 2
4. 1 2 2 1
Which four quantities a, b, c and d are required to balance the equation ...
aCa(OH)_2(aq) + bHCl_(aq) ==> cCaCl_2(aq) + dH₂O_(l) ? [eq-46]
1. 1 2 1 1
2. 1 2 1 2
3. 2 1 1 2
4. 2 2 2 1
Which four quantities a, b, c and d are required to balance the equation ...
aAl(OH)_3(s) + bHCl_(aq) ==> cAlCl_3(aq) + dH₂O_(l) ? [eq-47]
1. 2 6 2 3
2. 1 6 2 6
3. 1 3 1 3
4. 2 3 2 3
Which four quantities a, b, c and d are required to balance the equation ...
aFe₂O_3(s) + bHCl_(aq) ==> cFeCl_3(aq) + dH₂O_(l) ? [eq-48]
1. 2 6 2 3
2. 1 6 2 6
3. 1 3 1 3
4. 1 6 2 3
Which four quantities a, b, c and d are required to balance the equation ...
aMgO_(s) + bHCl_(aq) ==> cMgCl_2(aq) + dH₂O_(l) ? [eq-49]
1. 1 2 1 1
2. 1 1 1 1
3. 2 2 1 2
4. 1 4 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aMg(OH)_2(s) + bH₂SO_4(aq) ==> cMgSO_4(aq) + dH₂O_(l) ? [eq-50]
1. 1 2 1 1
2. 1 1 1 2
3. 2 2 1 2
4. 1 4 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aLi₂O_(s) + bHCl_(aq) ==> cLiCl_(aq) + dH₂O_(l) ? [eq-51]
1. 1 2 1 1
2. 1 1 1 1
3. 1 2 2 1
4. 1 2 1 2
Which four quantities a, b, c and d are required to balance the equation ...
aKOH_(aq) + bH₂SO_4(aq) ==> cK₂SO_4(aq) + dH₂O_(l) ? [eq-52]
1. 1 2 1 1
2. 1 1 1 1
3. 2 2 1 2
4. 2 1 1 2
Given the following symbol equation:
2Mg + O₂ ==> 2MgO
Calculate how many g of magnesium oxide is formed by burning 24g of magnesium in air.
(Relative atomic masses, A_r: Mg = 24 and O = 16) [com-1]
1. 40
2. 16
3. 20
4. 80
Given the following symbol equation:
2Mg + O₂ ==> 2MgO
Calculate how many tonne of magnesium is needed to make 80 tonne of magnesium oxide.
(Relative atomic masses, A_r: Mg = 24 and O = 16) [com-2]
1. 96
2. 48
3. 24
4. 16
Given the following symbol equation:
CaCO_3(s) ==> CaO_(s) + CO_2(g)
Calculate how many kg of calcium carbonate is needed to make 56 kg of calcium oxide.
(Relative atomic masses, A_r: Ca = 40, C = 12 and O = 16) [com-3]
1. 50
2. 44
3. 100
4. 40
Given the following symbol equation:
CaCO_3(s) ==> CaO_(s) + CO_2(g)
Calculate how many g of carbon dioxide is formed if 25g of calcium carbonate is decomposed on heating to form 14g of calcium oxide.
(Relative atomic masses, A_r: Ca = 40, C = 12 and O = 16) [com-4]
1. 22
2. 44
3. 10
4. 11
Given the symbol equation to show the formation of iron sulfide:
Fe + S ==> FeS
Calculate the mass in g of iron sulfide formed when 5.6g of iron combines with 3.2g of sulfur.
(Relative atomic masses, A_r: Fe = 56 and S = 32) [com-5]
1. 8.8
2. 2.4
3. 5.6
4. 3.2
Given the symbol equation to show the formation of iron sulfide:
Fe + S ==> FeS
Calculate the mass in g of iron sulfide formed when 28g of iron combines with 16g of sulfur.
(Relative atomic masses, A_r: Fe = 56 and S = 32) [com-6]
1. 12
2. 44
3. 28
4. 16
Given the symbol equation to show the formation of calcium chloride by burning calcium in chlorine:
Ca_(s) + Cl_2(g) ==> CaCl_2(s)
Calculate the mass in g of calcium chloride formed when 20g of calcium combines with 35.5g of chlorine.
(Relative atomic masses, A_r: Ca = 40 and Cl = 35.5) [com-7]
1. 15.5
2. 70.0
3. 55.5
4. 17.5
Given the symbol equation to show the formation of calcium chloride by burning calcium in chlorine:
Ca_(s) + Cl_2(g) ==> CaCl_2(s)
Calculate the mass in g of chlorine needed when 40g of calcium forms 111g of calcium chloride.
(Relative atomic masses, A_r: Ca = 40 and Cl = 35.5) [com-8]
1. 80
2. 100
3. 151
4. 71
Given the symbol equation to show the formation of aluminium sulfide by heating a mixture of aluminium and sulfur:
2Al + 3S ==> Al₂S₃
How many g of sulfur is needed if 54g of aluminium is reacted to form 150g of aluminium sulfide?
(Relative atomic masses, A_r: Al = 27 and S = 32) [com-9]
1. 96
2. 204
3. 64
4. 27
Given the symbol equation to show the formation of aluminium sulfide by heating a mixture of aluminium and sulfur:
2Al + 3S ==> Al₂S₃
How many kg of sulfur is needed if 108kg of aluminium is reacted to form 300kg of aluminium sulfide?
(Relative atomic masses, A_r: Al = 27 and S = 32) [com-10]
1. 408
2. 192
3. 96
4. 32
Given the symbol equation to show the formation of iron sulfide by heating a mixture of iron and sulfur:
Fe + S ==> FeS
Calculate the mass in g of iron unreacted when 60g of iron reacts with 32g of sulfur to form 88g of iron sulfide.
(Relative atomic masses, A_r: Fe = 56 and S = 32) [com-11]
1. 8
2. 32
3. 4
4. 56
Given the symbol equation to show the formation of iron sulfide by heating a mixture of iron and sulfur:
Fe + S ==> FeS
Calculate the mass in g of sulfur unreacted when 28g of iron reacts with 22g of sulfur to form 44g of iron sulfide.
(Relative atomic masses, A_r: Fe = 56 and S = 32) [com-12]
1. 22
2. 16
3. 12
4. 6
Given the symbol equation to show the formation of calcium chloride by burning calcium in chlorine:
Ca_(s) + Cl_2(g) ==> CaCl_2(s)
Calculate the mass in g of calcium left unreacted when 25g of calcium reacts with 35.5g of chlorine.
(Relative atomic masses, A_r: Ca = 40 and Cl = 35.5) [com-13]
1. 10.5
2. 5.0
3. 7.1
4. 12.5
Given the symbol equation to show the formation of calcium chloride by burning calcium in chlorine:
Ca_(s) + Cl_2(g) ==> CaCl_2(s)
Calculate the mass in g of chlorine left unreacted when 80g of calcium reacts with 150g of chlorine to form 222g of calcium chloride.
(Relative atomic masses, A_r: Ca = 40 and Cl = 35.5) [com-14]
1. 70
2. 8
3. 16
4. 72
Which of the following is a test for hydrogen gas? [gt1]
1. Gives a squeaky pop with a lit splint.
2. Relights a glowing red splint.
3. Turns blue litmus red then bleaches it white.
4. Turns red litmus paper blue
5. Gives a milky white precipitate with limewater (calcium hydroxide solution).
Which of the following is a test for oxygen gas? [gt2]
1. Gives a squeaky pop with a lit splint.
2. Relights a glowing red splint.
3. Turns blue litmus red then bleaches it white.
4. Turns red litmus paper blue
5. Gives a milky white precipitate with limewater (calcium hydroxide solution).
Which of the following is a test for chlorine gas? [gt3]
1. Gives a squeaky pop with a lit splint.
2. Relights a glowing red splint.
3. Turns blue litmus red then bleaches it white.
4. Turns red litmus paper blue
5. Gives a milky white precipitate with limewater (calcium hydroxide solution).
Which of the following is a test for ammonia gas? [gt4]
1. Gives a squeaky pop with a lit splint.
2. Relights a glowing red splint.
3. Turns blue litmus red then bleaches it white.
4. Turns red litmus paper blue
5. Gives a milky white precipitate with limewater (calcium hydroxide solution).
Which of the following is a test for carbon dioxide gas? [gt5]
1. Gives a squeaky pop with a lit splint.
2. Relights a glowing red splint.
3. Turns blue litmus red then bleaches it white.
4. Turns red litmus paper blue
5. Gives a milky white precipitate with limewater (calcium hydroxide solution).
Given the following relative atomic masses: Cu = 64, S = 32 and O = 16; calculate the relative formula mass of copper sulfate, CuSO₄ [rfm-1]
1. 160
2. 112
3. 96
4. 336
Given the following relative atomic masses: H = 1 and C = 12; calculate the relative molecular mass of ethane, C₂H₆ [rfm-2]
1. 13
2. 30
3. 18
4. 25
Given the following relative atomic masses: H = 1 and C = 12; calculate the relative molecular mass of octane, C₈H₁₈ [rfm-3]
1. 13
2. 96
3. 114
4. 112
Given the following relative atomic masses: H = 1, N = 14 and O = 16; calculate the relative formula mass of nitric acid, HNO₃ [rfm-4]
1. 31
2. 93
3. 62
4. 63
Given the following relative atomic masses: H = 1, N = 14 and O = 16; calculate the relative formula mass of ammonium nitrate, NH₄NO₃ [rfm-5]
1. 80
2. 31
3. 90
4. 180
Given the following relative atomic masses: H = 1, N = 14, O = 16 and S = 32; calculate the relative formula mass of ammonium sulfate, (NH₄)₂SO₄ [rfm-6]
1. 63
2. 132
3. 216
4. 100
Given the following relative atomic masses: H = 1, O = 16 and S = 32; calculate the relative formula mass of sulfuric acid, H₂SO₄ [rfm-7]
1. 49
2. 194
3. 98
4. 66
Given the following relative atomic masses: O = 16, Al = 27 and S = 32; calculate the relative formula mass of aluminium sulfate, Al₂(SO₄)₃ [rfm-8]
1. 75
2. 315
3. 171
4. 342
Given the following relative atomic masses: H = 1 and Cl = 35.5, calculate the relative formula mass of hydrochloric acid, HCl [rfm-9]
1. 36.5
2. 18
3. 35.5
4. 37.5
Given the following relative atomic masses: Na = 23 and Cl = 35.5, calculate the relative formula mass of sodium chloride, NaCl [rfm-10]
1. 40
2. 58.5
3. 49.5
4. 35
Given the following relative atomic masses: Ca = 40 and Cl = 35.5, calculate the relative formula mass of calcium chloride, CaCl₂ [rfm-11]
1. 75.5
2. 151
3. 111
4. 146.5
Given the following relative atomic masses: H = 1, O = 16 and Mg = 24, calculate the relative formula mass of magnesium hydroxide, Mg(OH)₂ [rfm-12]
1. 41
2. 82
3. 42
4. 58
Given the following relative atomic masses: Al = 27 and Cl = 35.5, calculate the relative formula mass of aluminium chloride, AlCl₃ [rfm-13]
1. 133.5
2. 62.5
3. 187.5
4. 98
Given the following relative atomic masses: H = 1, O = 16 and Al = 27, calculate the relative formula mass of aluminium hydroxide, Al(OH)₃ [rfm-14]
1. 44
2. 78
3. 132
4. 46
Given the following relative atomic masses: H = 1, C = 12 and O = 16; calculate the relative molecular mass of glucose, C₆H₁₂O₆ [rfm-5]
1. 29
2. 40
3. 180
4. 90
Given the following relative atomic masses: H = 1, C = 12 and O = 16; calculate the relative molecular mass of ethanol ('alcohol'), C₂H₅OH [rfm-16]
1. 29
2. 23
3. 41
4. 46
Given the following relative atomic masses: H = 1, C = 12 and O = 16; calculate the relative molecular mass of ethanoic acid ('acetic acid'), CH₃COOH [rfm-17]
1. 60
2. 29
3. 84
4. 58
Given the following relative atomic masses: O = 16 and Fe = 56; calculate the relative formula mass of iron(II) oxide, FeO [rfm-18]
1. 40
2. 72
3. 56
4. 16
Given the following relative atomic masses: O = 16 and Fe = 56; calculate the relative formula mass of iron(III) oxide, Fe₂O₃ [rfm-19]
1. 72
2. 200
3. 160
4. 216
Given the following relative atomic masses: O = 16 and Fe = 56; calculate the relative formula mass of the iron oxide, Fe₃O₄ [rfm-20]
1. 72
2. 272
3. 174
4. 232
Given the following relative atomic masses: H = 1 and C = 12; calculate the relative molecular mass of methane, CH₄ [rfm-21]
1. 16
2. 13
3. 52
4. 10
Given the following relative atomic masses: H = 1 and C = 12; calculate the relative molecular mass of propane, C₃H₈ [rfm-22]
1. 13
2. 44
3. 99
4. 40
Given the following relative atomic masses: C = 12 and O = 16; calculate the relative molecular mass of carbon dioxide, CO₂ [rfm-23]
1. 28
2. 56
3. 44
4. 14
Given the following relative atomic masses: C = 12, O = 16 and Cu = 64; calculate the relative formula mass of copper carbonate, CuCO₃ [rfm-24]
1. 92
2. 276
3. 148
4. 124
Given the following relative atomic masses: C = 12, O = 16 and Ca = 40; calculate the relative formula mass of calcium carbonate, CaCO₃ [rfm-25]
1. 100
2. 68
3. 204
4. 124
Given the equation: 2Mg_(s) + O_2(g) ==> 2MgO_(s)
and the atomic masses: Mg = 24, O = 16, how many g of magnesium is needed to make 10g of magnesium oxide? [rmc-1]
1. 6.0
2. 3.0
3. 1.2
4. 2.4
Given the equation: 2Mg_(s) + O_2(g) ==> 2MgO_(s)
and the atomic masses: Mg = 24, O = 16, how many tonne of magnesium oxide can be made from 3 tonne of magnesium? [rmc-2]
1. 2.4
2. 5.0
3. 8.0
4. 4.8
Given the equation: 2Mg_(s) + O_2(g) ==> 2MgO_(s)
and the atomic masses: Mg = 24, O = 16, what mass of oxygen in g, combines with 240g of magnesium? [rmc-3]
1. 64
2. 80
3. 160
4. 32
Iron sulfide can be made by heating an iron and sulfur mixture.
Fe_(s) + S_(s) ==> FeS_(s)
Given the atomic masses: Fe = 56, S = 32, how many g of iron sulfide can be made from 14g of iron? [rmc-4]
1. 44
2. 28
3. 16
4. 22
Iron sulfide can be made by heating an iron and sulfur mixture.
Fe_(s) + S_(s) ==> FeS_(s)
Given the atomic masses: Fe = 56, S = 32, how many g of sulfur reacts with 224g of iron? [rmc-5]
1. 128
2. 32
3. 64
4. 112
Iron sulfide can be made by heating an iron and sulfur mixture.
Fe_(s) + S_(s) ==> FeS_(s)
Given the atomic masses: Fe = 56, S = 32, how many g of iron is needed to make 440g of iron sulfide? [rmc-6]
1. 56
2. 280
3. 220
4. 168
The iron ore Haematite consists mainly of iron(III) oxide. In a blast furnace it is reduced to iron with carbon monoxide ...
Fe₂O_3(s) + 3CO_(g) ==> 2Fe_(l) + 3CO_2(g)
Given the atomic masses: Fe = 56, O =16, C=12, how many tonne of iron can be made from 40 tonnes of haematite ore? [rmc-7]
1. 56
2. 14
3. 28
4. 7
The iron ore Haematite consists mainly of iron(III) oxide. In a blast furnace it is reduced to iron with carbon monoxide ...
Fe₂O_3(s) + 3CO_(g) ==> 2Fe_(l) + 3CO_2(g)
Given the atomic masses: Fe = 56, O =16, C=12, how many tonne of haematite ore are needed to make 224 tonne of iron? [rmc-8]
1. 160
2. 480
3. 640
4. 320
The iron ore Haematite consists mainly of iron(III) oxide. In a blast furnace it is reduced to iron with carbon monoxide ...
Fe₂O_3(s) + 3CO_(g) ==> 2Fe_(l) + 3CO_2(g)
Given the atomic masses: Fe = 56, O =16, C=12, how g of carbon monoxide are needed to reduce 32g of iron oxide to iron? [rmc-9]
1. 16.8
2. 33.6
3. 8.4
4. 28.0
The iron ore Haematite consists mainly of iron(III) oxide. In a blast furnace it is reduced to iron with carbon monoxide ...
Fe₂O_3(s) + 3CO_(g) ==> 2Fe_(l) + 3CO_2(g)
Given the atomic masses: Fe = 56, O =16, C=12, how many g of carbon dioxide are formed when 80 g of haematite is reduced to iron? [rmc-10]
1. 44
2. 66
3. 33
4. 40
Lime (calcium oxide) is made by heating limestone (calcium carbonate).
CaCO_3(s) ==> CaO_(s) + CO_2(g)
Given the atomic masses: Ca = 40, C = 12, O = 16, how many tonne of limestone is needed to make 112 tonne of lime? [rmc-11]
1. 224
2. 400
3. 200
4. 300
Lime (calcium oxide) is made by heating limestone (calcium carbonate).
CaCO_3(s) ==> CaO_(s) + CO_2(g)
Given the atomic masses: Ca = 40, C = 12, O = 16, what mass in g of lime is made from 20g of limestone? [rmc-12]
1. 8.8
2. 5.6
3. 4.4
4. 11.2
Lime (calcium oxide) is made by heating limestone (calcium carbonate).
CaCO_3(s) ==> CaO_(s) + CO_2(g)
Given the atomic masses: Ca = 40, C = 12, O = 16, how many tonne of carbon dioxide is formed by decomposing 400 tonne of calcium carbonate? [rmc-13]
1. 176
2. 44
3. 88
4. 132
The salt zinc chloride can be made by dissolving zinc carbonate in dilute hydrochloric acid.
ZnCO_3(s) + 2HCl_(aq) ==> ZnCl_2(aq) + H₂O_(l) + CO_2(g)
Given the atomic masses: Zn = 65, C = 12, O =16, H = 1, Cl =35.5, how many g of zinc carbonate are needed to make 68g of zinc chloride?? [rmc-14]
1. 125.0
2. 62.5
3. 68.0
4. 136.0
The salt zinc chloride can be made by dissolving zinc carbonate in dilute hydrochloric acid.
ZnCO_3(s) + 2HCl_(aq) ==> ZnCl_2(aq) + H₂O_(l) + CO_2(g)
Given the atomic masses: Zn = 65, C = 12, O =16, H = 1, Cl =35.5, how many g of HCl are needed to make 408g of zinc chloride? [rmc-15]
1. 109.5
2. 36.5
3. 219.0
4. 71.0
The salt zinc chloride can be made by dissolving zinc carbonate in dilute hydrochloric acid.
ZnCO_3(s) + 2HCl_(aq) ==> ZnCl_2(aq) + H₂O_(l) + CO_2(g)
Given the atomic masses: Zn = 65, C = 12, O =16, H = 1, Cl =35.5, what mass of zinc chloride in g can be made from 25g of zinc carbonate? [rmc-16]
1. 54.4
2. 12.5
3. 13.6
4. 27.2
The salt zinc chloride can be made by dissolving zinc carbonate in dilute hydrochloric acid.
ZnCO_3(s) + 2HCl_(aq) ==> ZnCl_2(aq) + H₂O_(l) + CO_2(g)
Given the atomic masses: Zn = 65, C = 12, O =16, H = 1, Cl =35.5, how many g of water are formed when 250g of zinc carbonate reacts? [rmc-17]
1. 36
2. 18
3. 9
4. 27
The salt zinc chloride can be made by dissolving zinc carbonate in dilute hydrochloric acid.
ZnCO_3(s) + 2HCl_(aq) ==> ZnCl_2(aq) + H₂O_(l) + CO_2(g)
Given the atomic masses: Zn = 65, C = 12, O =16, H = 1, Cl =35.5, how many g of carbon dioxide are formed when 3.65g of hydrochloric acid reacts? [rmc-18]
1. 4.4
2. 2.2
3. 1.1
4. 8.8
The salt sodium sulfate, Na₂SO₄, can be made by neutralising sodium hydroxide with sulfuric acid.
2NaOH_(aq) + H₂SO_4(aq) ==> Na₂SO_4(aq) + 2H₂O_(l)
Given the atomic masses: Na = 23, O = 16, H = 1, S = 32, how many g of sodium hydroxide is needed to make 213g of sodium sulfate? [rmc-19]
1. 40
2. 80
3. 120
4. 160
The salt sodium sulfate, Na₂SO₄, can be made by neutralising sodium hydroxide with sulfuric acid.
2NaOH_(aq) + H₂SO_4(aq) ==> Na₂SO_4(aq) + 2H₂O_(l)
Given the atomic masses: Na = 23, O = 16, H = 1, S = 32, what mass in g of sulfuric acid is needed to make 7.1g of sodium sulfate? [rmc-20]
1. 9.8
2. 14.7
3. 19.6
4. 4.9
The salt sodium sulfate, Na₂SO₄, can be made by neutralising sodium hydroxide with sulfuric acid.
2NaOH_(aq) + H₂SO_4(aq) ==> Na₂SO_4(aq) + 2H₂O_(l)
Given the atomic masses: Na = 23, O = 16, H = 1, S = 32, how many g of sodium sulfate is formed when 8g of sodium hydroxide reacts? [rmc-21]
1. 14.2
2. 28.4
3. 7.1
4. 21.3
The salt sodium sulfate, Na₂SO₄, can be made by neutralising sodium hydroxide with sulfuric acid.
2NaOH_(aq) + H₂SO_4(aq) ==> Na₂SO_4(aq) + 2H₂O_(l)
Given the atomic masses: Na = 23, O = 16, H = 1, S = 32, how many g of water are formed when 49g of sulfuric acid reacts? [rmc-22]
1. 9
2. 18
3. 36
4. 23
Copper(I) sulfide ore can be converted to copper by roasting in air:
Cu₂S_(s) + O_2(g) ==> 2Cu_(s) + SO_2(g)
How many g of copper can be made from 320g of the copper ore?
(Relative atomic masses: Cu = 64, S = 32, O = 16) [rmc-23]
1. 128
2. 64
3. 256
4. 192
Copper(I) sulfide ore can be converted to copper by roasting in air:
Cu₂S_(s) + O_2(g) ==> 2Cu_(s) + SO_2(g)
How many tonnes of oxygen are needed to convert 40 tonnes of ore to copper?
(Relative atomic masses: Cu = 64, S = 32, O = 16) [rmc-24]
1. 16
2. 32
3. 12
4. 8
Copper(I) sulfide ore can be converted to copper by roasting in air:
Cu₂S_(s) + O_2(g) ==> 2Cu_(s) + SO_2(g)
How many tonnes of sulfur dioxide are produced for every 1280 tonnes of ore processed?
(Relative atomic masses: Cu = 64, S = 32, O = 16) [rmc-25]
1. 512
2. 128
3. 256
4. 64
Copper(I) sulfide ore can be converted to copper by roasting in air:
Cu₂S_(s) + O_2(g) ==> 2Cu_(s) + SO_2(g)
How many tonnes of ore are needed to make 25.6 tonnes of copper?
(Relative atomic masses: Cu = 64, S = 32, O = 16) [rmc-26]
1. 64
2. 32
3. 48
4. 56
Aluminium chloride can be prepared by passing dry chlorine or hydrogen chloride gas over heated aluminium metal. The equation for the hydrogen chloride reaction is:
2Al_(s) + 6HCl_(g) ==> 2AlCl_3(s) + 3H_2(g)
How many kg of aluminium chloride can be made from 27 kg of aluminium?
(Relative atomic masses: Al = 27.0, Cl = 35.5, H = 1.0) [rmc-27]
1. 267.0
2. 400.5
3. 133.5
4. 66.75
Aluminium chloride can be prepared by passing dry chlorine or hydrogen chloride gas over heated aluminium metal. The equation for the hydrogen chloride reaction is:
2Al_(s) + 6HCl_(g) ==> 2AlCl_3(s) + 3H_2(g)
How many tonnes of hydrogen would be produced by reacting 108 tonnes of aluminium?
(Relative atomic masses: Al = 27.0, Cl = 35.5, H = 1.0) [rmc-28]
1. 2
2. 3
3. 6
4. 12
Aluminium chloride can be prepared by passing dry chlorine or hydrogen chloride gas over heated aluminium metal. The equation for the chlorine reaction is:
2Al_(s) + 3Cl_2(g) ==> 2AlCl_3(s)
How much aluminium is needed to make 89 g of aluminium chloride?
(Relative atomic masses: Al = 27.0, Cl = 35.5, H =1) [rmc-29]
1. 18
2. 27
3. 54
4. 9
Aluminium chloride can be prepared by passing dry chlorine or hydrogen chloride gas over heated aluminium metal. The equation for the chlorine reaction is:
2Al_(s) + 3Cl_2(g) ==> 2AlCl_3(s)
How many tonne of chlorine is needed to make 1068 tonne of aluminium chloride?
(Relative atomic masses: Al = 27.0, Cl = 35.5, H = 1) [rmc-30]
1. 71
2. 852
3. 426
4. 213
Yellow lead(II) oxide ore can be reduced by heating with charcoal (carbon) in a furnace to give silvery liquid lead metal:
lead(II) oxide + carbon ==> lead + carbon dioxide
2PbO_(s) + C_(s) ==> 2Pb_(l) + CO_2(g)
How many tonne of lead can be made from 223 tonne of ore?
(Relative atomic masses: Pb = 207, O = 16, C = 12) [rmc-31]
1. 414.0
2. 103.5
3. 207.0
4. 310.5
Yellow lead(II) oxide ore can be reduced by heating with charcoal (carbon) in a furnace to give silvery liquid lead metal:
lead(II) oxide + carbon ==> lead + carbon dioxide
2PbO_(s) + C_(s) ==> 2Pb_(l) + CO_2(g)
How many tonne of ore is needed to make 828 tonne of lead?
(Relative atomic masses: Pb = 207, O = 16, C = 12) [rmc-32]
1. 223
2. 446
3. 1784
4. 892
Yellow lead(II) oxide ore can be reduced by heating with charcoal (carbon) in a furnace to give silvery liquid lead metal:
lead(II) oxide + carbon ==> lead + carbon dioxide
2PbO_(s) + C_(s) ==> 2Pb_(l) + CO_2(g)
How many kg of carbon is needed to make 828 kg of lead?
(Relative atomic masses: Pb = 207, O = 16, C = 12) [rmc-33]
1. 24
2. 12
3. 6
4. 48
Yellow lead(II) oxide ore can be reduced by heating with charcoal (carbon) in a furnace to give silvery liquid lead metal:
lead(II) oxide + carbon ==> lead + carbon dioxide
2PbO_(s) + C_(s) ==> 2Pb_(l) + CO_2(g)
How many g of carbon dioxide are formed when 207 g of lead are produced?
(Relative atomic masses: Pb = 207, O = 16, C = 12) [rmc-34]
1. 44
2. 22
3. 11
4. 33
Chlorine consists of 75% chlorine-35 and 25% chlorine-37. Calculate the A_r of chlorine to 3sf/1dp. [ram-1]
1. 35.5
2. 35.0
3. 36.0
4. 35.6
Bromine consists of the isotopes: 50.5% Br-79 and 49.5% Br-81. Calculate the relative atomic mass, A_r, of bromine to 3sf/1dp. [ram-2]
1. 80.1
2. 80.0
3. 79.9
4. 79.8
Lithium consists of 7.4% lithium-6 and 92.6% lithium-7. Calculate the relative atomic mass, A_r, of lithium to 2sf/1dp. [ram-3]
1. 6.5
2. 6.7
3. 6.9
4. 6.6
Boron is 19.7% B-10 and 80.3% B-11. Calculate the relative atomic mass, A_r, of boron to 3sf/1dp. [ram-4]
1. 10.5
2. 10.9
3. 10.3
4. 10.8
Antimony (Sb) is 57.2% Sb-121 and 42.8% Sb-123. Calculate the A_r of Sb to 4sf/1dp. [ram-5]
1. 121.9
2. 122.0
3. 122.1
4. 121.2
Chromium has four stable isotopes. 4.31% Cr-50, 83.76% Cr-52, 9.55% Cr-53 and 2.38% Cr-54. Calculate the relative atomic mass, A_r, of chromium to 3sf/1dp. [ram-6]
1. 52.3
2. 52.1
3. 52.2
4. 52.5
Copper consists of 69.1% Cu-63 and 30.9% Cu-65. Calculate the relative atomic mass, A_r, of copper to 3sf/1dp. [ram-7]
1. 64.0
2. 63.3
3. 63.6
4. 64.5
Europium consists of 47.8% Eu-151 and 52.2% Eu-153. Calculate A_r(Eu) to 4sf/1dp. [ram-8]
1. 151.9
2. 152.2
3. 151.5
4. 152.0
Gallium is made up of 60.2% gallium-69 and 39.8% of gallium-71. Calculate the A_r of gallium to 3sf/1dp. [ram-9]
1. 69.8
2. 70.0
3. 69.9
4. 69.5
Iron has four stable isotopes.
5.8% Fe-54, 91.7% Fe-56, 2.2% Fe-57 and 0.3% Fe-58. Calculate the A_r of iron to 3sf/1dp. [ram-10]
1. 56.2
2. 55.9
3. 56.3
4. 56.1
Magnesium consists of 78.6% ²⁴Mg, 10.1% ²⁵Mg and 11.3% of ²⁶Mg. Calculate the relative atomic mass, A_r, of magnesium to 3sf/1dp. [ram-11]
1. 25.0
2. 24.7
3. 24.3
4. 24.1
Neon consists of 90.9% ²⁰Ne, 0.3% ²¹Ne and 8.8% ²²Ne. Calculate the relative atomic mass, A_r, of neon to 3sf/1dp. [ram-12]
1. 20.5
2. 20.1
3. 20.3
4. 20.2
Rhenium (Re) consists of 37.1% ¹⁸⁵Re and 62.9% ¹⁸⁷Re. Calculate the relative atomic mass, A_r, of rhenium to 4sf/1dp. [ram-13]
1. 186.3
2. 186.0
3. 185.6
4. 185.5
Rubidium consists of the stable isotopes: ⁸⁵Rb (72.2%) and ⁸⁷Rb (27.8%). Calculate A_r(Rb) to 3sf/1dp. [ram-14]
1. 86.0
2. 85.6
3. 85.9
4. 85.5
Thallium consists of 29.5% thallium-203 and 70.5% thallium-205. Calculate the relative atomic mass, A_r, of to 4sf/1dp. [ram-15]
1. 204.0
2. 204.2
3. 204.4
4. 204.1
Heat is taken in when ammonium nitrate dissolves in water. This is an example of? [et-1]
1. electrolysis
2. endothermic charge
3. exothermic change
4. thermal decomposition
Change 1. When calcium carbonate forms calcium oxide and carbon dioxide heat is absorbed.
Change 2. Calcium oxide releases heat when shaken with carbon dioxide.
Which line BEST describes these changes? [et-2]
1. change 1 is endothermic; change 2 is exothermic
2. change 1 is exothermic; change 2 is endothermic
3. change 1 is exothermic; change 2 is exothermic
4. change 1 is endothermic; change 2 is endothermic
When sodium hydroxide dissolves in water the temperature rises. This is an example of? [et-3]
1. electrolysis
2. endothermic charge
3. exothermic change
4. thermal decomposition
The breaking of bonds in a chlorine molecule must be? [et-4]
1. electrolytic
2. endothermic
3. equilibrium
4. exothermic
The making of bonds in forming a hydrogen molecule from hydrogen atoms must be? [et-5]
1. electrolytic
2. endothermic
3. equilibrium
4. exothermic
Change 1. Water is added to blue cobalt chloride, it turns pink and heats up.
Change 2. When pink cobalt chloride is heated, water is driven off, it turns blue and takes in heat.
Which line BEST describes these changes? [et-12]
1. change 1 is endothermic; change 2 is endothermic
2. change 1 is exothermic; change 2 is exothermic
3. change 1 is exothermic; change 2 is endothermic
4. change 1 is endothermic; change 2 is exothermic
Which of the following statements BEST explains why a chemical reaction involving a catalyst goes faster than without the catalyst? [et-22]
1. the catalyst decreases the energy of collisions between reactant particles
2. the catalyst increases the frequency of collisions between reactant particles
3. the catalyst decreases the activation energy for the reaction
4. the catalyst increases the activation energy for the reaction
Which of the following statements BEST explains why a chemical reaction goes slower without a suitable catalyst? [et-23]
1. the catalyst increases the energy of collisions between reactant particles
2. the catalyst increases the frequency of collisions between reactant particles
3. the activation energy is higher for the catalysed reaction
4. the activation energy is higher for the uncatalysed reaction
When ammonium chloride dissolves in water the temperature falls. The type of energy change is described as? [et-24]
1. a decomposition
2. endothermic
3. exothermic
4. activated
When magnesium dissolves in hydrochloric acid the temperature rises. The type of energy change is described as? [et-25]
1. a decomposition
2. endothermic
3. exothermic
4. activated
The reaction between sulfuric acid and zinc is exothermic. During the reaction, which observation is correct? [et-26]
1. a precipitate forms
2. the temperature of the solution decreases
3. the temperature of the solution does not change
4. the temperature of the solution rises
Which of these processes is always exothermic? [et-27]
1. burning
2. evaporation
3. insulation
4. melting
Which of these processes is always exothermic? [et-28]
1. combustion
2. evaporation
3. insulation
4. melting
Which of these process is always endothermic? [et-29]
1. burning
2. condensation
3. evaporation
4. freezing
Which of these process is always endothermic? [et-30]
1. burning
2. condensation
3. freezing
4. melting
Which of these process is always endothermic? [et-31]
1. burning
2. boiling
3. condensation
4. freezing
Which of these process is always exothermic? [et-32]
1. boiling
2. condensing
3. evaporation
4. melting
Which of these process is always exothermic? [et-33]
1. boiling
2. evaporating
3. freezing
4. melting
The chemical change when a fuel burns can be described as? [et-34]
1. an endothermic reaction
2. an exothermic reaction
3. a precipitation
4. a reversible reaction
When ammonium nitrate is added to water, an endothermic reaction occurs and? [et-35]
1. heat is given out
2. the surroundings get hotter
3. the temperature falls
4. the temperature rises
Equal amounts of four different substances (A-D) where added separately to equal amounts of an acid and a thermometer placed in the mixture. For which substance is the reaction the most exothermic? [et-36]
1. temperature rises by 3^oC
2. temperature rises by 5^oC
3. temperature falls by 3^oC
4. temperature falls by 5^oC
Equal amounts of four different substances (A-D) where added separately to equal amounts of an acid and a thermometer placed in the mixture. For which substance is the reaction the most endothermic? [et-37]
1. temperature rises by 3^oC
2. temperature rises by 5^oC
3. temperature falls by 3^oC
4. temperature falls by 5^oC
Equal amounts of four different substances (A-D) where added separately to equal amounts of an acid and a thermometer placed in the mixture. For which substance is the reaction the least exothermic? [et-38]
1. temperature rises by 3^oC
2. temperature rises by 5^oC
3. temperature falls by 3^oC
4. temperature falls by 5^oC
Equal amounts of four different substances (A-D) where added separately to equal amounts of an acid and a thermometer placed in the mixture. For which substance is the reaction the least endothermic? [et-39]
1. temperature rises by 3^oC
2. temperature rises by 5^oC
3. temperature falls by 3^oC
4. temperature falls by 5^oC
Which of the following energy changes corresponds to the activation energy required for the forward reaction to take place? [et-40]
1. energy change 1
2. energy change 2
3. energy change 3
4. energy change 4
Which of the following energy changes corresponds to the overall energy change for the reaction? [et-42]
1. energy change 1
2. energy change 2
3. energy change 3
4. energy change 4
Which of the following energy changes corresponds to the activation energy required for the forward reaction to take place? [et-43]
1. energy change 1
2. energy change 2
3. energy change 3
4. energy change 4
Which of the following energy changes corresponds to the overall energy change for the reaction? [et-45]
1. energy change 1
2. energy change 2
3. energy change 3
4. energy change 4
When an exothermic reaction takes place, the reaction mixture gets hotter because? [et-46]
1. energy is always released in a chemical change which makes new substances
2. exothermic changes always produce gases
3. in an exothermic change the products are less stable than the reactants
4. more energy is released when new bonds are made than is needed to break existing bonds
When an exothermic reaction takes place, the reaction mixture gets hotter because? [et-47]
1. energy is always released in a chemical change which makes new substances
2. exothermic changes always produce gases
3. in an exothermic change the products are more stable than the reactants
4. more energy is absorbed when new bonds are made than is needed to break existing bonds
When an endothermic reaction takes place, the reaction mixture takes in heat because? [et-48]
1. energy is always absorbed in a chemical change which makes new substances
2. endothermic changes always produce energy
3. in an endothermic change the products are more stable than the reactants
4. more energy is absorbed when existing bonds are broken than is given out when new bonds are formed in the products
When an endothermic reaction takes place, the reaction mixture takes in heat because? [et-49]
1. energy is always absorbed in a chemical change which makes new substances
2. endothermic changes always produce energy
3. in an endothermic change the products are less stable than the reactants
4. more energy is released when new bonds are formed than is taken in when existing bonds in the reactants are broken
Energy is needed to make a mixture of methane and oxygen react. The mixture explodes when a lighted splint is applied. What type of energy is supplied by the splint? [et-50]
1. Activation energy
2. Catalyst energy
3. Kinetic energy
4. Renewable energy
Which of these involves a chemical reaction? [et-82]
1. baking bread : 2. boiling water : 3. corroding metals
1. 1 and 2
2. 1 and 3
3. 2 and 3
4. All of them
Which of the following is a chemical change? [et-83]
1. cooling a cup of tea
2. dissolving sugar in coffee
3. lighting a match
4. melting an ice-cube
Which of the following is a physical change? [et-84]
1. dissolving sugar in coffee
2. lighting a match
3. making lime from limestone
4. making polythene from gaseous oil molecules
Which of the following involves a chemical reaction? [et-85]
1. cooking a cake
2. filtering sand from water
3. fractionally distilling oil
4. melting ice
Which of the following results in a chemical reaction? [et-86]
1. adding vinegar to water
2. leaving milk to go sour
3. mixing salt with water
4. stirring sugar with tea
Which of these involves a chemical reaction? [et-87]
1. apples decaying
2. ice melting
3. magnetising iron
4. boiling water
Which of these involves a physical change and NOT a chemical reaction? [et-88]
1. apples decaying
2. frying bacon
3. iron rusting
4. boiling water
Which of these involves a physical change and NOT a chemical reaction? [et-89]
1. apples decaying
2. frying bacon
3. iron rusting
4. freezing water
Which of these involves a chemical reaction? [et-90]
1. crushing apples
2. toasting bread
3. magnetising iron
4. freezing water
Which of these results in chemical change? [et-91]
1. adding lime to vinegar
2. adding milk to tea
3. mixing salt with water
4. mixing iron and sulfur powders
Which of these results ONLY in a physical change? [et-92]
1. adding lime to vinegar
2. leaving bread to go mouldy
3. mixing salt with water
4. adding magnesium to hydrochloric acid
Which of the following temperature changes is NOT the result of a chemical change? [et-93]
1. a fall in temperature as liquid metal cools to solidify
2. a fall in temperature as a precipitate falls
3. a rise in temperature as neutralisation takes place
4. a rise in temperature when a fuel burns
The reaction between hydrogen and chlorine to form hydrogen chloride can be written as:
H₂(g) + Cl₂(g) ===> 2HCl(g)
Use the bond energies shown to calculate the energy change that takes place when hydrogen chloride is formed according to the above equation. (Bond energies in kJ/mol: H-H 435, Cl-Cl 245, H-Cl 430) [et-6]
1. 90 kJ given out
2. 180 kJ given out
3. 125 kJ taken in
4. 250 kJ taken in
The reaction between hydrogen and fluorine to form hydrogen fluoride can be written as
H₂(g) + F₂(g) ===> 2HF(g)
Use the bond energies shown to calculate the energy change that takes place when hydrogen fluoride is formed according to the above equation. (Bond energies in kJ/mol: H-H 435, F-F 155, H-F 560) [et-7]
1. 15 kJ taken in
2. 30 kJ taken in
3. 265 kJ given out
4. 530 kJ given out
The diagram below shows the reaction profile for the course of a chemical reaction. Which of the following statements is TRUE? [et-8]
1. The reaction is exothermic with an activation energy of 130 kJ/mol
2. The reaction is exothermic and 460 kJ/mol of heat energy is given out
3. The reaction is endothermic with an activation energy of 970 kJ/mol
4. The reaction is endothermic with 460 kJ/mol of heat taken in
The diagram below shows the reaction profile for the course of a chemical reaction. Which of the following statements is TRUE? [et-9]
1. The reaction is exothermic with an activation energy of 970 kJ/mol
2. The reaction is exothermic and 380 kJ/mol of heat energy is given out
3. The reaction is endothermic with an activation energy of 970 kJ/mol
4. The reaction is endothermic with 460 kJ/mol of heat taken in
The diagram below shows the reaction profile for the course of a chemical reaction. Which of the following statements is TRUE? [et-10]
1. The reaction is exothermic with an activation energy of 860 kJ/mol
2. The reaction is exothermic and 380 kJ/mol of heat energy is given out
3. The reaction is endothermic with an activation energy of 310 kJ/mol
4. The reaction is endothermic with 460 kJ/mol of heat taken in
The diagram below shows the reaction profile for the course of a chemical reaction. Which of the following statements is true? [et-11]
1. The reaction is exothermic with an activation energy of 860 kJ/mol
2. The reaction is exothermic and 770 kJ/mol of heat energy is given out
3. The reaction is endothermic with an activation energy of 860 kJ/mol
4. The reaction is endothermic with 220 kJ/mol of heat taken in
The chemical equation shows how water is formed from its elements.
2H₂ + O₂ ==> 2H₂O
The bond energies in kJ/mol are: H-H 440; O=O 500; H-O 460
How much energy is released when two moles of water are formed? [et-13]
1. 460 kJ
2. 480 kJ
3. 920 kJ
4. 2300 kJ
The reaction between hydrogen and bromine to form hydrogen bromide can be written as
H₂(g) + Br₂(g) ===> 2HBr(g)
Use the bond energies shown to calculate the energy change that takes place when hydrogen bromide is formed according to the above equation. (Bond energies in kJ/mol: H-H 435; Br-Br 200; H-Br 370) [et-14]
1. 105 kJ given out
2. 105 kJ taken in
3. 270 kJ given out
4. 270 kJ taken in
Which of the following reaction profiles represents an exothermic reaction with no activation energy? [et-15]
Which of the following reaction profiles represents an endothermic reaction with no activation energy? [et-16]
Which of the following reaction profiles represents a reaction with an activation energy but with no overall energy change? [et-17]
Which of the following reaction profiles represents an exothermic reaction with a small activation energy? [et-18]
Which of the following reaction profiles represents an endothermic reaction with a large activation energy? [et-19]
Which of the following reaction profiles represents an exothermic reaction with a large activation energy? [et-20]
Which of the following reaction profiles represents an endothermic reaction with a small activation energy? [et-21]
Which of the following energy changes corresponds to the activation energy required for the reverse or backward reaction to take place? [et-41]
1. energy change 1
2. energy change 2
3. energy change 3
4. energy change 4
Which of the following energy changes corresponds to the activation energy required for the reverse or backward reaction to take place? [et-44]
1. energy change 1
2. energy change 2
3. energy change 3
4. energy change 4
An energy level diagram can be used to show the energy changes involved in the course of a chemical reaction. The reaction must be? [et-51]
1. an exothermic reaction
2. a thermal decomposition
3. an endothermic reaction
4. a reaction with zero activation energy
An energy level diagram can be used to show the energy changes involved in the course of a chemical reaction. The reaction must be? [et-52]
1. a combustion reaction
2. a thermal decomposition
3. an endothermic reaction
4. a reaction with zero activation energy
An energy level diagram can be used to show the energy changes involved in the course of a chemical reaction. The reaction must be? [et-53]
1. an exothermic reaction
2. a combustion reaction
3. an endothermic reaction
4. a reaction with zero activation energy
The diagram shows the energy changes during a reaction. What would occur if a catalyst was used?[et-54]
1. energy change 1 is lowered
2. energy change 2 is raised
3. energy change 3 is lowered
4. energy change 4 is raised
The diagram shows the energy changes during a reaction. What would occur if a catalyst was used?[et-55]
1. energy change 1 is lowered
2. energy change 2 is raised
3. energy change 3 is lowered
4. energy change 4 is raised
The diagram shows the profile of the energy changes for a reaction. Which energy change is reduced by using a suitable catalyst? [et-56]
1. energy change 1
2. energy change 2
3. energy change 3
4. energy change 4
The diagram shows the profile of the energy changes for a reaction. Which energy change is reduced by using a suitable catalyst? [et-57]
1. energy change 1
2. energy change 2
3. energy change 3
4. energy change 4
The diagram shows the profile of the energy changes for a reaction. Which energy change represents the energy needed to break chemical bonds so that new products can form? [et-58]
1. energy change 1
2. energy change 2
3. energy change 3
4. energy change 4
The diagram shows the profile of the energy changes for a reaction. Which energy change represents the energy needed to break chemical bonds so that new products can form? [et-59]
1. energy change 1
2. energy change 2
3. energy change 3
4. energy change 4
For the reaction: 3H₂ + N₂ ==> 2NH₃
The breaking of bonds in a hydrogen molecule when it combines with nitrogen to form ammonia must be? [et-60]
1. electrolytic
2. electrostatic
3. endothermic
4. exothermic
For the reaction: 3H₂ + N₂ ==> 2NH₃
The breaking of bonds in a nitrogen molecule when it combines with hydrogen to form ammonia must be? [et-61]
1. electrolytic
2. electrostatic
3. endothermic
4. exothermic
For the reaction: 3H₂ + N₂ ==> 2NH₃
The forming of bonds in an ammonia molecule when hydrogen combines with nitrogen must be? [et-62]
1. electrolytic
2. electrostatic
3. endothermic
4. exothermic
The equation for the formation of ammonia from its elements is:
3H₂ + N₂ ==> 2NH₃
Given the BOND ENERGIES in kJ/mol for H-H = 440; N-N = 940; N-H = 390, calculate the energy released when 2 moles of ammonia are formed. [et-63]
1. 80 kJ
2. 90 kJ
3. 990 kJ
4. 1110 kJ
The reaction between hydrogen and iodine to form hydrogen iodide can be written as
H₂(g) + I₂(g) ===> 2HI(g)
Use the bond energies shown to calculate the energy change that takes place when hydrogen iodide is formed according to the above equation. (Bond energies in kJ/mol: H-H 440, I-I 150, H-I 300) [et-64]
1. 10 kJ given out
2. 10 kJ taken in
3. 600 kJ given out
4. 590 kJ taken in
When hydrogen fluoride is heated it breaks down into hydrogen and fluorine.
The equation can be written as: 2HF_(g) ==> H_2(g) + F_2(g)
Use the bond energies shown below to calculate the energy change that takes place when 2 moles of hydrogen fluoride thermally decomposes in this way. (bond energies in kJ/mol: H-H = 440; F-F = 155; H-F = 560) [et-65]
1. 525 kJ taken in
2. 525 kJ given out
3. 560 kJ given out
4. 560 kJ taken in
When hydrogen chloride is heated it breaks down into hydrogen and fluorine.
The equation can be written as: 2HCl_(g) ==> H_2(g) + Cl_2(g)
Use the bond energies shown below to calculate the energy change that takes place when 2 moles of hydrogen chloride thermally decomposes in this way. (bond energies in kJ/mol: H-H = 440; Cl-Cl = 245; H-Cl = 430) [et-66]
1. 175 kJ given out
2. 175 kJ taken in
3. 860 kJ given out
4. 685 kJ taken in
When hydrogen bromide is heated it breaks down into hydrogen and bromine.
The equation can be written as: 2HBr_(g) ==> H_2(g) + Br_2(g)
Use the bond energies shown below to calculate the energy change that takes place when 2 moles of hydrogen bromide thermally decomposes in this way. (bond energies in kJ/mol: H-H = 440; Br-Br = 200; H-Br = 370) [et-67]
1. 740 kJ given out
2. 640 kJ taken in
3. 100 kJ taken in
4. 100 kJ given out
When hydrogen iodide is heated it breaks down into hydrogen and iodine.
The equation can be written as: 2HI_(g) ==> H_2(g) + I_2(g)
Use the bond energies shown below to calculate the energy change that takes place when 2 moles of hydrogen iodide thermally decomposes in this way. (bond energies in kJ/mol: H-H = 440; I-I = 150; H-I = 300) [et-68]
1. 600 kJ given out
2. 600 kJ taken in
3. 10 kJ given out
4. 10 kJ taken in
Methane molecules, CH₄, can be broken down into gaseous carbon and hydrogen atoms. The energy needed to break the bonds to do this is 1664 kJ/mol. Therefore the average C-H bond energy in the molecule is? [et-69]
1. 416 kJ
2. 832 kJ
3. 1664 kJ
4. 6656 kJ
Ammonia molecules, NH₃, can be broken down into gaseous nitrogen and hydrogen atoms. The energy needed to break the bonds to do this is 1164 kJ/mol. Therefore the average N-H bond energy in the molecule is? [et-70]
1. 388 kJ
2. 582 kJ
3. 1164 kJ
4. 291 kJ
Water molecules, H₂O, can be broken down into gaseous oxygen and hydrogen atoms. The energy needed to break the bonds to do this is 928 kJ/mol. Therefore the average O-H bond energy in the molecule is? [et-71]
1. 116 kJ
2. 232 kJ
3. 464 kJ
4. 928 kJ
The diagram shows the energy changes as a reaction proceeds. For a reaction to be exothermic which of the following must be positive? [et-72]
1. Y + X - W
2. Y - X + W
3. W - Y
4. X - Y
The diagram shows the energy changes as a reaction proceeds. Which of the following is the activation energy? [et-73]
1. W - X
2. W + X - Y
3. W - Y
4. X - Y
The diagram shows the energy changes as a reaction proceeds. Which of the following is the overall energy change? [et-74]
1. W - X given out
2. W - X taken in
3. X - Y given out
4. X - Y taken in
The diagram shows the energy changes as a reaction proceeds. For a reaction to be endothermic which of the following must be positive? [et-75]
1. W - X
2. W - Y
3. W + X - Y
4. X - Y
The diagram shows the energy changes as a reaction proceeds. Which of the following is the activation energy? [et-76]
1. Y + X - W
2. Y - X + W
3. X - Y
4. W - Y
The diagram shows the energy changes as a reaction proceeds. Which of the following is the overall energy change? [et-77]
1. X - Y given out
2. W - Y taken in
3. X - Y given out
4. X - Y taken in
Sodium hydroxide and dilute hydrochloric acid react together to form sodium chloride without being heated. This is because the? [et-78]
1. the activation energy is high
2. the activation energy is low
3. the activation energy is zero
4. the reaction is exothermic
Natural gas and the oxygen in air will only react when heated. This is because the reaction? [et-79]
1. has a zero activation energy
2. has a low activation energy
3. is exothermic
4. has a high activation energy
The diagram shows the energy changes as a reaction proceeds. If a suitable catalyst is used, which of the following energy changes occurs? [et-80]
1. W - X is increased
2. W - X is reduced
3. X - Y is increased
4. X - Y is reduced
The diagram shows the energy changes as a reaction proceeds. If a suitable catalyst is used, which of the following energy changes occurs? [et-81]
1. W - X is increased
2. W - Y is reduced
3. X - Y is increased
4. X - Y is reduced
Which of the following is a 'combustion reaction'? [rt-1]
1. CH_4(g) + 2O_2(g) => CO_2(g) + 2H₂O_(l)
2. NaOH_(aq) + HCl_(aq) => NaCl_(aq) + H₂O_(l)
3. CaCO_3(s) => CaO_(s) + CO_2(g)
4. C₆H₁₂O_6(aq) ==> 2C₂H₅OH_(aq) + 2CO_2(g)
Which of the following is a 'neutralisation reaction'? [rt-2]
1. CH_4(g) + 2O_2(g) => CO_2(g) + 2H₂O_(l)
2. NaOH_(aq) + HCl_(aq) => NaCl_(aq) + H₂O_(l)
3. CaCO_3(s) => CaO_(s) + CO_2(g)
4. C₆H₁₂O_6(aq) ==> 2C₂H₅OH_(aq) + 2CO_2(g)
Which of the following is a 'thermal decomposition' reaction? [rt-3]
1. CH_4(g) + 2O_2(g) => CO_2(g) + 2H₂O_(l)
2. NaOH_(aq) + HCl_(aq) => NaCl_(aq) + H₂O_(l)
3. CaCO_3(s) => CaO_(s) + CO_2(g)
4. C₆H₁₂O_6(aq) ==> 2C₂H₅OH_(aq) + 2CO_2(g)
Which of the following is a 'fermentation' reaction? [rt-4]
1. CH_4(g) + 2O_2(g) => CO_2(g) + 2H₂O_(l)
2. NaOH_(aq) + HCl_(aq) => NaCl_(aq) + H₂O_(l)
3. CaCO_3(s) => CaO_(s) + CO_2(g)
4. C₆H₁₂O_6(aq) ==> 2C₂H₅OH_(aq) + 2CO_2(g)
Which of the following is a 'combustion' reaction? [rt-5]
1. methane + oxygen => carbon dioxide + water
2. sodium hydroxide + hydrochloric acid => sodium chloride + water
3. calcium carbonate => calcium oxide + carbon dioxide
4. glucose => ethanol + carbon dioxide
Which of the following is a 'neutralisation' reaction? [rt-6]
1. methane + oxygen => carbon dioxide + water
2. sodium hydroxide + hydrochloric acid => sodium chloride + water
3. calcium carbonate => calcium oxide + carbon dioxide
4. glucose => ethanol + carbon dioxide
Which of the following is a 'thermal decomposition' reaction? [rt-7]
1. methane + oxygen => carbon dioxide + water
2. sodium hydroxide + hydrochloric acid => sodium chloride + water
3. calcium carbonate => calcium oxide + carbon dioxide
4. glucose => ethanol + carbon dioxide
Which of the following is a 'fermentation' reaction? [rt-8]
1. methane + oxygen => carbon dioxide + water
2. sodium hydroxide + hydrochloric acid => sodium chloride + water
3. calcium carbonate => calcium oxide + carbon dioxide
4. glucose => ethanol + carbon dioxide
Which is a 'neutralisation' reaction to form a soluble salt? [rt-9]
1. CuO_(s) + H₂SO_4(aq) => CuSO_4(aq) + H₂O_(l)
2. 2Al_(s) + Fe₂O_3(s) => 2Fe_(s) + Al₂O_3(s)
3. C₆H_14(g) => C₂H_4(g) + C₄H_10(g)
4. Ca(OH)_2(aq) + CO_2(g) => CaCO_3(s) + H₂O_(l)
Which of the following reactions is the 'Thermit reaction'? [rt-10]
1. CuO_(s) + H₂SO_4(aq) => CuSO_4(aq) + H₂O_(l)
2. 2Al_(s) + Fe₂O_3(s) => 2Fe_(s) + Al₂O_3(s)
3. C₆H_14(g) => C₂H_4(g) + C₄H_10(g)
4. Ca(OH)_2(aq) + CO_2(g) => CaCO_3(s) + H₂O_(l)
Which of the following reactions is a 'cracking' reaction? [rt-11]
1. CuO_(s) + H₂SO_4(aq) => CuSO_4(aq) + H₂O_(l)
2. 2Al_(s) + Fe₂O_3(s) => 2Fe_(s) + Al₂O_3(s)
3. C₆H_14(g) => C₂H_4(g) + C₄H_10(g)
4. Ca(OH)_2(aq) + CO_2(g) => CaCO_3(s) + H₂O_(l)
Which of the following reactions is a 'precipitation' reaction? [rt-12]
1. CuO_(s) + H₂SO_4(aq) => CuSO_4(aq) + H₂O_(l)
2. 2Al_(s) + Fe₂O_3(s) => 2Fe_(s) + Al₂O_3(s)
3. C₆H_14(g) => C₂H_4(g) + C₄H_10(g)
4. Ca(OH)_2(aq) + CO_2(g) => CaCO_3(s) + H₂O_(l)
Which is a 'neutralisation' reaction to form a soluble salt? [rt-13]
1. copper(II) oxide + sulfuric acid => copper(II) sulfate + water
2. aluminium + iron(III) oxide => aluminium oxide + iron
3. hexane => ethene + butane
4. calcium hydroxide + carbon dioxide => calcium carbonate + water
Which of the following reactions is the 'Thermit reaction? [rt-14]
1. copper(II) oxide + sulfuric acid => copper(II) sulfate + water
2. aluminium + iron(III) oxide => aluminium oxide + iron
3. hexane => ethene + butane
4. calcium hydroxide + carbon dioxide => calcium carbonate + water
Which of the following reactions is a 'cracking' reaction? [rt-15]
1. copper(II) oxide + sulfuric acid => copper(II) sulfate + water
2. aluminium + iron(III) oxide => aluminium oxide + iron
3. hexane => ethene + butane
4. calcium hydroxide + carbon dioxide => calcium carbonate + water
Which of the following reactions is a 'precipitation' reaction? [rt-16]
1. copper(II) oxide + sulfuric acid => copper(II) sulfate + water
2. aluminium + iron(III) oxide => aluminium oxide + iron
3. hexane => ethene + butane
4. calcium hydroxide + carbon dioxide => calcium carbonate + water
Which of the following is a 'displacement' reaction? [rt-17]
1. Mg_(s) + CuSO_4(aq) ==> Cu_(s) + MgSO_4(aq)
2. C₆H_14(g) => C₂H_4(g) + C₄H_10(g)
3. C₆H₁₂O_6(aq) + 6O_2(g) ==> 6CO_2(g) + 6H₂O_(l)
4. Na₂SO_4(aq) + BaCl_2(aq) ==> 2NaCl_(aq) + BaSO_4(aq)
Which of the following is a 'thermal decomposition'? [rt-18]
1. Mg_(s) + CuSO_4(aq) ==> Cu_(s) + MgSO_4(aq)
2. C₆H_14(g) => C₂H_4(g) + C₄H_10(g)
3. C₆H₁₂O_6(aq) + 6O_2(g) ==> 6CO_2(g) + 6H₂O_(l)
4. Na₂SO_4(aq) + BaCl_2(aq) ==> 2NaCl_(aq) + BaSO_4(aq)
Which of the following represents 'respiration'? [rt-19]
1. Mg_(s) + CuSO_4(aq) ==> Cu_(s) + MgSO_4(aq)
2. C₆H_14(g) => C₂H_4(g) + C₄H_10(g)
3. C₆H₁₂O_6(aq) + 6O_2(g) ==> 6CO_2(g) + 6H₂O_(l)
4. Na₂SO_4(aq) + BaCl_2(aq) ==> 2NaCl_(aq) + BaSO_4(aq)
Which of the following is a 'double decomposition'? [rt-20]
1. Mg_(s) + CuSO_4(aq) ==> Cu_(s) + MgSO_4(aq)
2. C₆H_14(g) => C₂H_4(g) + C₄H_10(g)
3. C₆H₁₂O_6(aq) + 6O_2(g) ==> 6CO_2(g) + 6H₂O_(l)
4. Na₂SO_4(aq) + BaCl_2(aq) ==> 2NaCl_(aq) + BaSO_4(aq)
Which of the following is a 'displacement' reaction? [rt-21]
1. magnesium + copper sulfate ==> copper + magnesium sulfate
2. hexane ==> ethene + butane
3. glucose + oxygen ==> carbon dioxide + water
4. sodium sulfate + barium chloride ==> sodium chloride + barium sulfate
Which of the following is a 'thermal decomposition'? [rt-22]
1. magnesium + copper sulfate ==> copper + magnesium sulfate
2. hexane ==> ethene + butane
3. glucose + oxygen ==> carbon dioxide + water
4. sodium sulfate + barium chloride ==> sodium chloride + barium sulfate
Which of the following represents 'respiration'? [rt-23]
1. magnesium + copper sulfate ==> copper + magnesium sulfate
2. hexane ==> ethene + butane
3. glucose + oxygen ==> carbon dioxide + water
4. sodium sulfate + barium chloride ==> sodium chloride + barium sulfate
Which of the following is a 'double decomposition'? [rt-24]
1. magnesium + copper sulfate ==> copper + magnesium sulfate
2. hexane ==> ethene + butane
3. glucose + oxygen ==> carbon dioxide + water
4. sodium sulfate + barium chloride ==> sodium chloride + barium sulfate
Which of A to D represents 'photosynthesis'? [rt-25]
1. 6CO_2(g) + 6H₂O_(l) ==> C₆H₁₂O_6(aq) + 6O_2(g)
2. n CH₂=CH₂ ==> (-CH₂-CH₂-)_n
3. N_2(g) + 3H_2(g) 2NH_3(g)
4. CH_4(g) + 2O_2(g) ==> CO_2(g) + 2H₂O_(l)
Which of A to D represents a 'polymerisation' reaction? [rt-26]
1. 6CO_2(g) + 6H₂O_(l) ==> C₆H₁₂O_6(aq) + 6O_2(g)
2. n CH₂=CH₂ ==> (-CH₂-CH₂-)_n
3. N_2(g) + 3H_2(g) 2NH_3(g)
4. CH_4(g) + 2O_2(g) ==> CO_2(g) + 2H₂O_(l)
Which of A to D represents a 'reversible' reaction? [rt-27]
1. 6CO_2(g) + 6H₂O_(l) ==> C₆H₁₂O_6(aq) + 6O_2(g)
2. n CH₂=CH₂ ==> (-CH₂-CH₂-)_n
3. N_2(g) + 3H_2(g) 2NH_3(g)
4. CH_4(g) + 2O_2(g) ==> CO_2(g) + 2H₂O_(l)
Which of A to D represents a 'burning' reaction? [rt-28]
1. 6CO_2(g) + 6H₂O_(l) ==> C₆H₁₂O_6(aq) + 6O_2(g)
2. n CH₂=CH₂ ==> (-CH₂-CH₂-)_n
3. N_2(g) + 3H_2(g) 2NH_3(g)
4. CH_4(g) + 2O_2(g) ==> CO_2(g) + 2H₂O_(l)
Which of A to D represents 'photosynthesis'? [rt-29]
1. carbon dioxide + water ==> glucose + oxygen
2. ethene ==> poly(ethene)
3. nitrogen + hydrogen ammonia
4. methane + oxygen ==> carbon dioxide + water
Which of A to D represents a 'plastic forming' reaction? [rt-30]
1. carbon dioxide + water ==> glucose + oxygen
2. ethene ==> poly(ethene)
3. nitrogen + hydrogen ammonia
4. methane + oxygen ==> carbon dioxide + water
Which of A to D represents a 'reversible' reaction? [rt-31]
1. carbon dioxide + water ==> glucose + oxygen
2. ethene ==> poly(ethene)
3. nitrogen + hydrogen ammonia
4. methane + oxygen ==> carbon dioxide + water
Which of A to D represents a 'burning' reaction? [rt-32]
1. carbon dioxide + water ==> glucose + oxygen
2. ethene ==> poly(ethene)
3. nitrogen + hydrogen ammonia
4. methane + oxygen ==> carbon dioxide + water
Which description means an 'EXOTHERMIC REACTION'? [rt-33]
1. heat is given out by the reaction
2. heat is taken in by the reaction
3. the reaction readily changes direction if the conditions are changed
4. the reaction continues in both directions but no concentrations change
Which description means an 'ENDOTHERMIC REACTION'? [rt-34]
1. heat is given out by the reaction
2. heat is taken in by the reaction
3. the reaction readily changes direction if the conditions are changed
4. the reaction continues in both directions but no concentrations change
Which description means a 'REVERSIBLE REACTION'? [rt-35]
1. heat is given out by the reaction
2. heat is taken in by the reaction
3. the reaction readily changes direction if the conditions are changed
4. the reaction stops in both directions and no concentrations change
Which description means a 'CHEMICAL EQUILIBRIUM'? [rt-36]
1. heat is given out by the reaction
2. heat is taken in by the reaction
3. the reaction readily changes direction if the conditions are changed
4. the reaction continues in both directions but no concentrations change
Which of the following is an ENDOTHERMIC chemical change? [rt-37]
1. calcium carbonate => calcium oxide + carbon dioxide
2. methane + oxygen => carbon dioxide + water
3. sodium hydroxide + hydrochloric acid => sodium chloride + water
4. glucose + oxygen => water + carbon dioxide
Which of the following is an ENDOTHERMIC chemical change? [rt-38]
1. methane + oxygen => carbon dioxide + water
2. hexane => ethane + propene
3. sodium hydroxide + hydrochloric acid => sodium chloride + water
4. glucose + oxygen => water + carbon dioxide
Which of the following is an ENDOTHERMIC chemical change? [rt-39]
1. sodium hydroxide + hydrochloric acid => sodium chloride + water
2. methane + oxygen => carbon dioxide + water
3. water + carbon dioxide => glucose + oxygen
4. glucose + oxygen => water + carbon dioxide
Which of the following is an ENDOTHERMIC chemical change? [rt-40]
1. sodium hydroxide + hydrochloric acid => sodium chloride + water
2. methane + oxygen => carbon dioxide + water
3. glucose + oxygen => water + carbon dioxide
4. sodium chloride => sodium + chlorine
Which of the following is an EXOTHERMIC chemical change? [rt-41]
1. sodium hydroxide + hydrochloric acid => sodium chloride + water
2. calcium carbonate => calcium oxide + carbon dioxide
3. hexane => ethane + propene
4. water + carbon dioxide => glucose + oxygen
Which of the following is an EXOTHERMIC chemical change? [rt-42]
1. calcium carbonate => calcium oxide + carbon dioxide
2. methane + oxygen => carbon dioxide + water
3. hexane => ethane + propene
4. water + carbon dioxide => glucose + oxygen
Which of the following is an EXOTHERMIC chemical change? [rt-43]
1. calcium carbonate => calcium oxide + carbon dioxide
2. hexane => ethane + propene
3. glucose + oxygen => water + carbon dioxide
4. sodium chloride => sodium + chlorine
Which of the following is an EXOTHERMIC chemical change? [rt-44]
1. calcium carbonate => calcium oxide + carbon dioxide
2. hexane => ethane + propene
3. water + carbon dioxide => glucose + oxygen
4. sodium + chlorine => sodium chloride
Which ionic equation is an 'acid-alkali neutralisation'? [rt-45]
1. H⁺_(aq) + OH^-_(aq) ==> H₂O_(l)
2. MgO_(s) + 2H⁺_(aq) ==> Mg²⁺_(aq) + H₂O_(l)
3. Ag⁺_(aq) + Cl^-_(aq) ==> AgCl_(s)
4. Zn_(s) + Cu²⁺_(aq) ==> Zn²⁺_(aq) + Cu_(s)
Which ionic equation is an 'acid-insoluble base neutralisation'? [rt-46]
1. H⁺_(aq) + OH^-_(aq) ==> H₂O_(l)
2. MgO_(s) + 2H⁺_(aq) ==> Mg²⁺_(aq) + H₂O_(l)
3. Ag⁺_(aq) + Cl^-_(aq) ==> AgCl_(s)
4. Zn_(s) + Cu²⁺_(aq) ==> Zn²⁺_(aq) + Cu_(s)
Which ionic equation corresponds to a 'non-redox precipitation reaction'? [rt-47]
1. H⁺_(aq) + OH^-_(aq) ==> H₂O_(l)
2. MgO_(s) + 2H⁺_(aq) ==> Mg²⁺_(aq) + H₂O_(l)
3. Ag⁺_(aq) + Cl^-_(aq) ==> AgCl_(s)
4. Zn_(s) + Cu²⁺_(aq) ==> Zn²⁺_(aq) + Cu_(s)
Which ionic equation corresponds to a 'redox reaction'? [rt-48]
1. H⁺_(aq) + OH^-_(aq) ==> H₂O_(l)
2. MgO_(s) + 2H⁺_(aq) ==> Mg²⁺_(aq) + H₂O_(l)
3. Ag⁺_(aq) + Cl^-_(aq) ==> AgCl_(s)
4. Zn_(s) + Cu²⁺_(aq) ==> Zn²⁺_(aq) + Cu_(s)
Which of the following represents a 'reduction only' change? [rt-49]
1. Cu²⁺_(aq) + 2e^- ==> Cu_(s)
2. Zn_(s) - 2e^- ==> Zn²⁺_(s)
3. Mg_(s) + Fe²⁺_(aq) ==> Mg²⁺_(aq) + Fe_(s)
4. 2Cl^-_(aq) - 2e^- ==> Cl_{2 (g)}
Which of the following represents an 'oxidation only' change? [rt-50]
1. Cu²⁺_(aq) + 2e^- ==> Cu_(s)
2. Zn_(s) - 2e^- ==> Zn²⁺_(s)
3. Mg_(s) + Fe²⁺_(aq) ==> Mg²⁺_(aq) + Fe_(s)
4. Cl_{2 (aq)} +2e^- ==> 2Cl^-_(aq)
Which of the following is a 'redox' reaction? [rt-51]
1. Cu²⁺_(aq) + 2e^- ==> Cu_(s)
2. Cl_{2 (aq)} +2e^- ==> 2Cl^-_(aq)
3. Mg_(s) + Fe²⁺_(aq) ==> Mg²⁺_(aq) + Fe_(s)
4. 2Cl^-_(aq) - 2e^- ==> Cl_{2 (g)}
Which of the following represents an 'oxidation only' change? [rt-52]
1. Cu²⁺_(aq) + 2e^- ==> Cu_(s)
2. Br_{2 (aq)} + 2e^- ==> 2Br^-_(aq)
3. Mg_(s) + Fe²⁺_(aq) ==> Mg²⁺_(aq) + Fe_(s)
4. 2Cl^-_(aq) - 2e^- ==> Cl_{2 (g)}
Which of the following is a 'redox' reaction? [rt-53]
1. Cl_{2 (aq)} + 2I^-_(aq) ==> 2Cl^-_(aq) + I_{2 (aq)}
2. Br_{2 (aq)} + 2e^- ==> 2Br^-_(aq)
3. Ag⁺_(aq) + Cl^-_(aq) ==> AgCl_(s)
4. H⁺_(aq) + OH^-_(aq) ==> H₂O_(l)
Which is a 'reduction only' reaction? [rt-54]
1. Cl_{2 (aq)} + 2I^-_(aq) ==> 2Cl^-_(aq) + I_{2 (aq)}
2. Br_{2 (aq)} + 2e^- ==> 2Br^-_(aq)
3. Ag⁺_(aq) + Cl^-_(aq) ==> AgCl_(s)
4. H⁺_(aq) + OH^-_(aq) ==> H₂O_(l)
Which does 'NOT involve an oxidation or reduction' reaction? [rt-55]
1. Cl_{2 (aq)} + 2I^-_(aq) ==> 2Cl^-_(aq) + I_{2 (aq)}
2. Br_{2 (aq)} + 2e^- ==> 2Br^-_(aq)
3. Ag⁺_(aq) + Cl^-_(aq) ==> AgCl_(s)
4. Mg_(s) + Fe²⁺_(aq) ==> Mg²⁺_(aq) + Fe_(s)
Which of the following does'NOT involve an oxidation or reduction' reaction? [rt-56]
1. Cl_{2 (aq)} + 2I^-_(aq) ==> 2Cl^-_(aq) + I_{2 (aq)}
2. Br_{2 (aq)} + 2e^- ==> 2Br^-_(aq)
3. Zn_(s) - 2e^- ==> Zn²⁺_(s)
4. H⁺_(aq) + OH^-_(aq) ==> H₂O_(l)
For the following reaction: Fe₂O₃ + 3CO ==> 2Fe + 3CO₂
Which is 'reduced? [rt-57]
1. Fe₂O₃
2. CO
3. Fe
4. CO₂
For the following reaction: Fe₂O₃ + 3CO ==> 2Fe + 3CO₂
Which is 'oxidised? [rt-58]
1. Fe₂O₃
2. CO
3. Fe
4. CO₂
For the following reaction: Fe₂O₃ + 3CO ==> 2Fe + 3CO₂
Which acts as an 'oxidising agent? [rt-59]
1. Fe
2. CO₂
3. Fe₂O₃
4. CO
For the following reaction: Fe₂O₃ + 3CO ==> 2Fe + 3CO₂
Which acts as an 'reducing agent? [rt-60]
1. Fe
2. CO₂
3. Fe₂O₃
4. CO
Which of the following corresponds to the 'Haber Synthesis'? [rt-61]
1. N_{2 (g)} + 3H_{2 (g)} ==> 2NH_{3 (g)}
2. 2SO_{2 (g)} + O_{2 (g)} ==> 2SO_{3 (g)}
3. CaCO_{3 (s)} => CaO_(s) + CO_{2 (g)}
4. 2CO_(g) + 2NO_(g) ==> 2CO_{2 (g)} + N_{2 (g)}
Which of the following corresponds to the 'Contact Process'? [rt-62]
1. N_{2 (g)} + 3H_{2 (g)} ==> 2NH_{3 (g)}
2. 2SO_{2 (g)} + O_{2 (g)} ==> 2SO_{3 (g)}
3. CaCO_{3 (s)} => CaO_(s) + CO_{2 (g)}
4. 2CO_(g) + 2NO_(g) ==> 2CO_{2 (g)} + N_{2 (g)}
Which of the following corresponds to the 'limekiln reaction'? [rt-63]
1. N_{2 (g)} + 3H_{2 (g)} ==> 2NH_{3 (g)}
2. 2SO_{2 (g)} + O_{2 (g)} ==> 2SO_{3 (g)}
3. CaCO_{3 (s)} => CaO_(s) + CO_{2 (g)}
4. 2CO_(g) + 2NO_(g) ==> 2CO_{2 (g)} + N_{2 (g)}
Which of the following corresponds to 'catalytic conversion' in a car exhaust? [rt-64]
1. N_{2 (g)} + 3H_{2 (g)} ==> 2NH_{3 (g)}
2. 2SO_{2 (g)} + O_{2 (g)} ==> 2SO_{3 (g)}
3. CaCO_{3 (s)} => CaO_(s) + CO_{2 (g)}
4. 2CO_(g) + 2NO_(g) ==> 2CO_{2 (g)} + N_{2 (g)}
For the reaction: copper(II) oxide + hydrogen ==> copper + water
... which of the following is 'reduced'? [rt-65]
1. copper(II) oxide
2. hydrogen
3. copper
4. water
For the reaction: copper(II) oxide + hydrogen ==> copper + water
... which of the following is 'oxidised'? [rt-66]
1. copper(II) oxide
2. hydrogen
3. copper
4. water
For the reaction: copper(II) oxide + hydrogen ==> copper + water
... which of the following acts as the 'oxidising agent'? [rt-67]
1. copper
2. water
3. copper(II) oxide
4. hydrogen
For the reaction: copper(II) oxide + hydrogen ==> copper + water
... which of the following acts as the 'reducing agent'? [rt-68]
1. copper
2. water
3. copper(II) oxide
4. hydrogen
Which of the following corresponds to 'a hydration reaction'? [rt-69]
1. ethene + water ==> ethanol (using acid catalyst)
2. blue copper sulfate ==> white copper sulfate + water (on heating the salt)
3. sugar solution ==> ethanol + carbon dioxide (using yeast)
4. methane + oxygen ==> carbon dioxide + water (burning reaction)
Which of the following corresponds to 'a dehydration reaction'? [rt-70]
1. ethene + water ==> ethanol (using acid catalyst)
2. blue copper sulfate ==> white copper sulfate + water (on heating the salt)
3. sugar solution ==> ethanol + carbon dioxide (using yeast)
4. methane + oxygen ==> carbon dioxide + water (burning reaction)
Which of the following corresponds to 'a dehydration reaction'? [rt-71]
1. ethene + water ==> ethanol (using acid catalyst)
2. sugar solution ==> ethanol + carbon dioxide (using yeast)
3. sugar ==> carbon + water (using concentrated sulfuric acid)
4. methane + oxygen ==> carbon dioxide + water (burning reaction)
Which of the following corresponds to 'a dehydration reaction'? [rt-72]
1. sodium hydroxide + hydrochloric acid ==> sodium chloride + water (neutralisation)
2. sugar solution ==> ethanol + carbon dioxide (using yeast)
3. methane + oxygen ==> carbon dioxide + water (burning reaction)
4. ethanol ==> ethene + water (using acid catalyst)
Which of the following corresponds to 'a hydration reaction'? [rt-73]
1. white copper sulfate + water ==> blue copper sulfate (adding cold water)
2. sugar solution ==> ethanol + carbon dioxide (using yeast)
3. methane + oxygen ==> carbon dioxide + water (burning reaction)
4. ethanol ==> ethene + water (using acid catalyst)
Which of the following corresponds to 'a hydration reaction'? [rt-74]
1. CuSO₄.5H₂O ==> CuSO₄ + 5H₂O
2. CH₂=CH₂ + H₂O ==> CH₃CH₂OH
3. C₆H₁₂O₆ ==> 2CH₃CH₂OH + 2CO₂
4. C₆H₁₂O₆ ==> 6C + 6H₂O
Which of the following corresponds to 'a dehydration reaction'? [rt-75]
1. C₆H₁₂O₆ ==> 2CH₃CH₂OH + 2CO₂
2. CH₂=CH₂ + H₂O ==> CH₃CH₂OH
3. CuSO₄.5H₂O ==> CuSO₄ + 5H₂O
4. CH₄ + 2O₂ ==> CO₂ + 2H₂O
Which of the following corresponds to 'a dehydration reaction'? [rt-76]
1. C₆H₁₂O₆ ==> 2CH₃CH₂OH + 2CO₂
2. CH₂=CH₂ + H₂O ==> CH₃CH₂OH
3. CH₄ + 2O₂ ==> CO₂ + 2H₂O
4. C₆H₁₂O₆ ==> 6C + 6H₂O
Which of the following corresponds to 'a dehydration reaction'? [rt-77]
1. CH₃CH₂OH ==> CH₂=CH₂ + H₂O
2. C₆H₁₂O₆ ==> 2CH₃CH₂OH + 2CO₂
3. CH₄ + 2O₂ ==> CO₂ + 2H₂O
4. CuSO₄ + 5H₂O ==> CuSO₄.5H₂O
Which of the following corresponds to 'a hydration reaction'? [rt-78]
1. CH₃CH₂OH ==> CH₂=CH₂ + H₂O
2. CuSO₄ + 5H₂O ==> CuSO₄.5H₂O
3. CH₄ + 2O₂ ==> CO₂ + 2H₂O
4. C₆H₁₂O₆ ==> 6C + 6H₂O
The reaction illustrated produces ...? [ab-1]
1. a salt + water
2. a salt only
3. a salt and hydrogen
4. water only
The type of reaction illustrated is called ...? [ab-2]
1. decomposition
2. neutralisation
3. displacement
4. oxidation
To produce sodium sulfate by the reaction illustrated you need ...? [ab-3]
1. potassium sulfate + sodium hydroxide
2. sodium chloride + sulfuric acid
3. sodium hydroxide + sulfuric acid
4. sodium hydroxide + hydrochloric acid
In the reaction illustrated, in order to add the correct amount of acid you would add a few drops of Universal Indicator and add acid until the indicator in the conical flask was ...? [ab-4]
1. blue
2. orange
3. yellow
4. green
In the reaction illustrated, in order to add the correct amount of acid you would add a few drops of Universal Indicator to the conical flask. If too little acid was added the indicator colour could be? [ab-5]
1. blue
2. orange
3. yellow
4. green
In the reaction illustrated, in order to add the correct amount of acid you would add a few drops of Universal Indicator to the conical flask. If too much acid was added the indicator colour could be? [ab-6]
1. blue
2. orange
3. purple
4. green
To produce potassium chloride by the reaction illustrated you need ...? [ab-7]
1. potassium sulfate + hydrochloric acid
2. sodium chloride + potassium hydroxide
3. potassium hydroxide + hydrochloric acid
4. sodium hydroxide + hydrochloric acid
To produce lithium nitrate by the reaction illustrated you need ...? [ab-8]
1. lithium sulfate + nitric acid
2. sodium nitrate + lithium hydroxide
3. potassium nitrate + lithium hydroxide
4. lithium hydroxide + nitric acid
The diagram shows a method of preparing salts.
Which of the following will forms when a transition metal oxide reacts with hydrochloric acid? [ab-9]
1. transition metal chloride + water
2. transition metal chloride + hydrogen
3. transition metal chloride only
4. water only
The diagram shows a method of preparing salts from reacting an insoluble metal oxide and an acid.
This type of reaction is called? [ab-10]
1. electrolysis
2. neutralisation
3. reduction
4. displacement
The diagram shows a method of preparing salts by reacting an insoluble metal oxide with an acid.
How can you tell when all the acid has been used up before filtering the mixture? [ab-11]
1. universal indicator will give a yellow colour in the acid
2. universal indicator will give a pale blue colour in the acid
3. no more of the metal oxide will dissolve in the acid
4. the solution will go clear
The diagram shows a method of preparing salts.
Which of the following will form a transition metal sulfate and hydrogen? [ab-12]
1. transition metal oxide + sulfuric acid
2. transition metal + sodium sulfate
3. transition metal hydroxide + potassium sulfate
4. transition metal + sulfuric acid
Which is the strongest base or alkali? [ab-13]
1. limewater
2. baking soda
3. vinegar
4. wine
Which is the weakest base or alkali? [ab-14]
1. limewater
2. baking soda
3. vinegar
4. wine
Which is the strongest acid? [ab-15]
1. limewater
2. baking soda
3. vinegar
4. wine
Which is the weakest acid? [ab-16]
1. limewater
2. baking soda
3. vinegar
4. wine
Which of the following can be mixed to form a neutral solution? [ab-17]
1. limewater and fizzy drink
2. baking soda and toothpaste
3. vinegar and wine
4. calomine lotion and common salt
Which of the following can be mixed to form a neutral solution? [ab-18]
1. limewater and washing soda
2. baking soda and wine
3. vinegar and common salt
4. ammonia and limewater
Which of the following can be safely used to treat an acid bee sting? [ab-19]
1. limewater
2. wine
3. calomine lotion
4. common salt
Which of the following can be safely used to treat an alkaline wasp sting? [ab-20]
1. calomine lotion
2. vinegar
3. washing soda
4. common salt
Which of the following is most likely to be part of an ant-acid indigestion medicine? [ab-21]
1. sodium hydrogencarbonate
2. ammonia
3. washing soda
4. limewater
Which of the following is the safest to use to treat an acid nettle sting? [ab-22]
1. wine
2. sodium hydrogencarbonate
3. washing soda
4. limewater
A small amount of a dense white powder was mixed with water in a test tube. Non of the white powder sank to the bottom of the test tube. A few drops of universal indicator were added and the solution turned blue. This meant the white powder was ...? [ab-23]
1. a soluble neutral substance
2. a slightly soluble acid
3. a very soluble alkali
4. a slightly soluble alkali
A small amount of a dense white powder was mixed with water in a test tube. Some of the white powder sank to the bottom of the test tube. A few drops of universal indicator were added and the solution turned blue. This meant the white powder was ...? [ab-24]
1. a soluble neutral substance
2. a slightly soluble acid
3. a very soluble alkali
4. a slightly soluble alkali
A small amount of a dense white powder was mixed with water in a test tube. Non of the white powder sank to the bottom of the test tube. A few drops of universal indicator were added and the solution turned green. This meant the white powder was ...? [ab-25]
1. a soluble neutral substance
2. a slightly soluble acid
3. a slightly soluble neutral substance
4. a slightly soluble alkali
A small amount of a dense white powder was mixed with water in a test tube. Some of the white powder sank to the bottom of the test tube. A few drops of universal indicator were added and the solution turned green. This meant the white powder was ...? [ab-26]
1. a soluble acidic substance
2. a slightly soluble neutral substance
3. a soluble acidic substance
4. a slightly soluble alkali
A small amount of a dense white powder was mixed with water in a test tube. Non of the white powder sank to the bottom of the test tube. A few drops of universal indicator were added and the solution turned orange. This meant the white powder was ...? [ab-26]
1. a soluble weak alkali
2. a very soluble neutral substance
3. a soluble weak acid
4. a slightly soluble strong acid
A small amount of a dense white powder was mixed with water in a test tube. Some of the white powder sank to the bottom of the test tube. A few drops of universal indicator were added and the solution turned red. This meant the white powder was ...? [ab-26]
1. a soluble weak alkali
2. a slightly soluble neutral substance
3. a soluble weak acid
4. a slightly soluble strong acid
Which of the following is the pH of a strong acid? [ab-49]
1. pH 1
2. pH 14
3. pH 5
4. pH 9
Which of the following is the pH of a strong alkali? [ab-50]
1. pH 1
2. pH 14
3. pH 5
4. pH 9
Which of the following is the pH of a weak acid? [ab-51]
1. pH 1
2. pH 14
3. pH 5
4. pH 9
Which of the following is the pH of a weak alkali? [ab-52]
1. pH 1
2. pH 14
3. pH 5
4. pH 9
When dilute nitric acid reacts with sodium hydroxide the products are? [ab-53]
1. sodium nitrate + water
2. sodium nitrate + hydrogen
3. sodium hydride + hydrogen nitrate
4. sodium nitrite + oxygen
dilute acid X + copper(II) carbonate ==> copper(II) sulfate + water + carbon dioxide. Acid X is? [ab-54]
1. nitric acid
2. sulfuric acid
3. sulfurous acid
4. hydrochloric acid
dilute acid X + magnesium hydroxide ==> magnesium chloride + water. Acid X is? [ab-55]
1. ammonium chlorate
2. sulfuric acid
3. hydrochloric acid
4. chloric acid
magnesium + dilute acid X ==> magnesium nitrate + hydrogen. Acid X is? [ab-56]
1. ammonium nitrate
2. nitrogen dioxide
3. nitrous acid
4. nitric acid
When hydrochloric acid is added to copper carbonate, the gas bubbles formed can be identified by? [ab-57]
1. burning with a squeaky pop
2. turning limewater cloudy
3. relighting a glowing splint
4. turning blue litmus red and then bleaching it
When sulfuric acid is added to zinc, the gas bubbles formed can be identified by? [ab-58]
1. burning with a squeaky pop
2. turning limewater cloudy
3. relighting a glowing splint
4. turning blue litmus red and then bleaching it
An iron tray was cleaned with dilute hydrochloric acid and bubbles formed. The gas formed was? [ab-59]
1. oxygen
2. chlorine
3. hydrogen
4. carbon dioxide
A carbonate mineral rock was tested with dilute sulfuric acid and bubbles formed. The gas formed was? [ab-60]
1. carbon monoxide
2. sulfur dioxide
3. hydrogen
4. carbon dioxide
Dilute sulfuric acid will only form one product when reacted with? [ab-61]
1. ammonia
2. copper
3. magnesium oxide
4. zinc carbonate
Dilute sulfuric acid will not readily react with? [ab-62]
1. ammonia
2. copper
3. magnesium oxide
4. zinc carbonate
Which will form a salt and water when reacted with dilute hydrochloric acid? [ab-63]
1. ammonia
2. copper
3. magnesium oxide
4. zinc carbonate
Which will form a salt, water and carbon dioxide when reacted with dilute hydrochloric acid? [ab-64]
1. ammonia
2. copper
3. magnesium oxide
4. zinc carbonate
Which of these reactants is the best combination to use to make magnesium sulfate? [ab-65]
1. magnesium oxide + sulfuric acid
2. magnesium chloride + sodium sulfate
3. sulfuric acid + magnesium chloride
4. magnesium nitrate + sulfuric acid
Which of these reactants is the best combination to use to make zinc nitrate? [ab-66]
1. zinc chloride + nitric acid
2. nitric acid + zinc hydroxide
3. nitric acid + zinc sulfate
4. zinc oxide + nitrous acid
Which of these reactants is the best combination to use to make copper(II) sulfate? [ab-67]
1. copper + sulfuric acid
2. copper(II) chloride + sodium sulfate
3. copper(II) oxide + sulfuric acid
4. copper(II) nitrate + sodium chloride
Which of these reactants is the best combination to use to make zinc chloride? [ab-68]
1. calcium chloride + zinc carbonate
2. zinc nitrate + hydrochloric acid
3. sodium chloride + zinc oxide
4. zinc carbonate + hydrochloric acid
The diagram shows the preparation of a salt. Which word applies to stages 1-2? [ab-69]
1. neutralisation
2. filtration
3. evaporation
4. condensation
The diagram shows the preparation of a salt. Which word applies to stage 3? [ab-70]
1. neutralisation
2. filtration
3. evaporation
4. condensation
The diagram shows the preparation of a salt. Which word describes the change from 3 to 4? [ab-71]
1. neutralisation
2. filtration
3. evaporation
4. condensation
The diagram shows the preparation of a salt. Which word describes stage 4? [ab-72]
1. neutralisation
2. filtration
3. evaporation
4. crystallisation
The diagram shows the preparation of a salt using a solid and an acid. Which is true concerning this method? [ab-73]
1. the solid can be an insoluble base
2. it is not a neutralisation reaction
3. you cannot use an insoluble carbonate
4. the solid must be an alkali
The diagram shows the preparation of a salt. Which word means a 'soluble base'? [ab-74]
1. oxide
2. alkali
3. hydroxide
4. indicator
The diagram shows a method of salt preparation. Which statement is true about the method? [ab-75]
1. the method uses an insoluble base
2. the acid must be in the burette and the alkali in the flask
3. the neutralisation point is detected with an indicator
4. the salt will precipitate at the neutralisation point
The diagram shows one method of salt preparation. Which statement is true about the method illustrated? [ab-76]
1. the salt will precipitate at the neutralisation point
2. an alkali is used
3. the neutralisation point is detected with an indicator
4. the method uses an insoluble base
Complete the word equation:
zinc oxide + hydrochloric acid ==> ..???.. [ab-77]
1. zinc chloride + hydrogen
2. zinc hydrochloride + water
3. zinc chloride + water
4. zinc hydrochloride chloride + water + carbon dioxide
Complete the word equation:
zinc hydroxide + hydrochloric acid ==> ..???.. [ab-78]
1. zinc hydrochloride + water
2. zinc chloride + water + carbon dioxide
3. zinc hydrochloride + hydrogen
4. zinc chloride + water
Complete the word equation:
zinc + hydrochloric acid ==> ..???.. [ab-79]
1. zinc chloride + hydrogen
2. zinc chloride + water
3. zinc hydrochloride + hydrogen
4. zinc hydrochloride + water
Complete the word equation:
zinc carbonate + hydrochloric acid ==> ..???.. [ab-80]
1. zinc hydrochloride + water
2. zinc chloride + water + carbon dioxide
3. zinc hydrochloride + hydrogen
4. zinc chloride + carbon dioxide
Complete the word equation:
nickel + sulfuric acid ==> ..???.. [ab-81]
1. nickel sulfate + hydrogen
2. nickel sulfate + water
3. nickel sulfite + water
4. nickel sulfite + hydrogen
Complete the word equation:
nickel oxide + sulfuric acid ==> ..???.. [ab-82]
1. nickel sulfate + hydrogen
2. nickel sulfate + water
3. nickel sulfite + water
4. nickel sulfite + hydrogen
Complete the word equation:
nickel hydroxide + sulfuric acid ==> ..???.. [ab-83]
1. nickel sulfate + hydrogen
2. nickel sulfite + water
3. nickel sulfate + water
4. nickel sulfite + hydrogen
Complete the word equation:
nickel carbonate + sulfuric acid ==> ..???.. [ab-84]
1. nickel sulfate + carbon dioxide
2. nickel sulfite + water
3. nickel sulfate + water
4. nickel sulfate + water + carbon dioxide
Complete the word equation:
ammonia + sulfuric acid ==> ..???.. [ab-85]
1. ammonium sulfate
2. ammonia sulfate
3. ammonium hydrogensulfate
4. ammonia sulfite
Complete the word equation:
ammonia + hydrochloric acid ==> ..???.. [ab-86]
1. ammonia chloride
2. ammonium chloride
3. ammonium hydrochloride
4. ammonia hydrochloride
Complete the word equation:
ammonia + nitric acid ==> ..???.. [ab-87]
1. ammonia nitrite
2. ammonium nitrite
3. ammonium nitrate
4. ammonia hydrogennitrate
Complete the word equation:
sodium hydroxide + sulfuric acid ===> ..???.. [ab-88]
1. sodium sulfate
2. sodium sulfate + hydrogen
3. sodium hydrogensulfite + water
4. sodium sulfate + water
Given the following neutralisation equation:
NaOH_(aq) + HCl_(aq) ==> NaCl_(aq) + H₂O_(l)
Which is the alkali? [ab-89]
1. NaOH
2. HCl
3. NaCl
4. H₂O
Given the following neutralisation equation:
NaOH_(aq) + HCl_(aq) ==> NaCl_(aq) + H₂O_(l)
Which is the acid? [ab-90]
1. NaOH
2. HCl
3. NaCl
4. H₂O
Given the following neutralisation equation:
NaOH_(aq) + HCl_(aq) ==> NaCl_(aq) + H₂O_(l)
Which is the salt? [ab-91]
1. NaOH
2. HCl
3. NaCl
4. H₂O
Given the following neutralisation equation:
NaOH_(aq) + HCl_(aq) ==> NaCl_(aq) + H₂O_(l)
Which is the base? [ab-92]
1. H₂O
2. HCl
3. NaCl
4. NaOH
Which two reactants would you use to make potassium nitrate? [ab-101]
1. nitric acid and potassium hydroxide
2. sodium nitrate and potassium chloride
3. sulfuric acid and sodium nitrate
4. nitric acid and sodium hydroxide
Insoluble metal oxides and metal hydroxides (bases) will not dissolve to form an alkaline solution. But they will dissolve in acids to give the same reaction as with alkalis. This method is particularly handy for making transition metal salts. Which reaction will produce a transition metal chloride and hydrogen? [ab-102]
1. transition metal oxide + sodium chloride
2. transition metal + hydrochloric acid
3. transition metal hydroxide + hydrochloric acid
4. transition metal + sulfuric acid
Insoluble metal oxides and metal hydroxides (bases) will not dissolve to form an alkaline solution. But they will dissolve in acids to give the same reaction as with alkalis. This method is particularly handy for making transition metal salts. When sufficient base has been added so that no more dissolves, how is the excess base removed? [ab-103]
1. boiling
2. distillation
3. filtration
4. crystallisation
Insoluble metal oxides and metal hydroxides (bases) will not dissolve to form an alkaline solution. But they will dissolve in acids to give the same reaction as with alkalis. This method is particularly handy for making transition metal salts. When sufficient base has been added so that no more dissolves. How could you test that all the acid was neutralised? [ab-104]
1. see if crystals form on evaporating the solution
2. see if the solution is clear
3. measure the boiling point of the solution
4. use indicator paper
Insoluble bases and metals will not dissolve to form an alkaline solution, but they will dissolve in acids to form salts. This method is particularly handy for making transition metal salts. What pair of chemicals will make cobalt sulfate and water? [ab-105]
1. cobalt oxide + sulfuric acid
2. cobalt + hydrochloric acid
3. cobalt + nitric acid
4. cobalt hydroxide + nitric acid
Insoluble bases and metals will not dissolve to form an alkaline solution, but they will dissolve in acids to form salts. This method is particularly handy for making transition metal salts. What pair of chemicals will make cobalt chloride and hydrogen? [ab-106]
1. cobalt oxide + sulfuric acid
2. cobalt + hydrochloric acid
3. cobalt hydroxide + sodium chloride
4. cobalt hydroxide + nitric acid
Which two reactants make ammonium chloride and water? [ab-107]
1. ammonium sulfate and hydrochloric acid
2. ammonium hydroxide and sodium chloride
3. ammonium hydroxide and hydrochloric acid
4. ammonia and potassium chloride
Which of these gives an alkaline solution when dissolved in water? [ab-108]
1. aluminium hydroxide
2. copper hydroxide
3. iron hydroxide
4. ammonia (ammonium hydroxide)
Which of these gives an alkaline solution when dissolved in water? [ab-109]
1. sodium hydroxide
2. copper hydroxide
3. iron hydroxide
4. aluminium hydroxide
Which of these gives an alkaline solution when dissolved in water? [ab-109]
1. nickel hydroxide
2. potassium hydroxide
3. iron hydroxide
4. magnesium hydroxide
Which of A to D completes the equation ..?.. [ab-111]
..?.. + potassium hydroxide ==> potassium sulfate + water
1. potassium nitrate
2. calcium hydroxide
3. sulfuric acid
4. sodium chloride
Which of A to D completes the equation ..?.. [ab-112]
hydrochloric acid + sodium hydroxide ==> ..?.. + water
1. sodium sulfate
2. potassium chloride
3. calcium chloride
4. sodium chloride
Which of A to D completes the equation ..?.. [ab-113]
..?.. + nitric acid ==> ammonium nitrate
1. ammonia (ammonium hydroxide)
2. calcium hydroxide
3. ammonium sulfate
4. sodium nitrate
Which of A to D completes the equation ..?.. [ab-114]
sulfuric acid + ..?.. ==> calcium sulfate + water
1. ammonia sulfate
2. calcium hydroxide
3. calcium chloride
4. sodium sulfate
Which quantities a, b, c and d are required to balance the equation ... (note that '1's would not be shown in the equation)
a Zn_(s) + b HCl_(aq) ==> c ZnCl_2(aq) + d H_2(g) ? [ab-29]
1. 1 2 1 1
2. 2 2 2 1
3. 2 1 1 2
4. 1 1 2 2
Which quantities a, b, c and d are required to balance the equation ... (note that '1's would not be shown in the equation)
a Fe_(s) + b H₂SO_4(aq) ==> c FeSO_4(aq) + d H_2(g) ? [ab-30]
1. 1 1 1 2
2. 1 1 1 1
3. 2 2 2 1
4. 2 1 2 2
Which quantities a, b, c and d are required to balance the equation ... (note that '1's would not be shown in the equation)
a Al_(s) + b HCl_(aq) ==> c AlCl_3(aq) + d H_2(g) ? [ab-31]
1. 1 6 3 2
2. 2 3 2 3
3. 2 6 2 3
4. 1 3 3 2
Which quantities a, b, c and d are required to balance the equation ... (note that '1's would not be shown in the equation)
a Al_(s) + b H₂SO_4(aq) ==> c Al₂(SO₄)_3(aq) + d H_2(g) ? [ab-32]
1. 1 3 1 3
2. 2 3 2 3
3. 1 2 2 2
4. 2 3 1 3
Which quantities a, b, c, d and e are required to balance the equation ... (note that '1's would not be shown in the equation)
a CaCO_3(s) + b HCl_(aq) ==> c CaCl_2(aq) + d H₂O_(l) + e CO_2(g) ? [ab-33]
1. 1 2 1 1 1
2. 2 2 1 2 1
3. 1 1 1 1 1
4. 2 1 2 2 2
Which quantities a, b, c, d and e are required to balance the equation ... (note that '1's would not be shown in the equation)
a Na₂CO_3(s) + b HCl_(aq) ==> c NaCl_(aq) + d H₂O_(l) + e CO_2(g) ? [ab-34]
1. 1 4 4 2 2
2. 1 2 2 1 1
3. 2 2 4 2 2
4. 2 2 2 1 1
Which quantities a, b, c, d and e are required to balance the equation ... (note that '1's would not be shown in the equation)
a Tl₂(CO₃)_3(s) + b HCl_(aq) ==> c TlCl_3(aq) + d H₂O_(l) + e CO_2(g) ? [ab-35]
1. 2 6 4 3 6
2. 1 3 2 6 2
3. 1 6 2 3 3
4. 2 3 4 3 6
Which quantities a, b, c, d and e are required to balance the equation ... (note that '1's would not be shown in the equation)
a Tl₂(CO₃)_3(s) + b H₂SO_4(aq) ==> c Tl₂(SO₄)_3(aq) + d H₂O_(l) + e CO_2(g) ? [ab-36]
1. 2 6 4 3 6
2. 1 3 2 6 6
3. 1 6 2 6 3
4. 1 3 1 3 3
Which quantities a, b, c and d are required to balance the equation ... (note that '1's would not be shown in the equation)
a NaOH_(aq) + b HCl_(aq) ==> c NaCl_(aq) + d H₂O_(l) ? [ab-37]
1. 1 1 1 1
2. 1 2 2 1
3. 2 1 1 2
4. 1 2 1 1
Which quantities a, b, c and d are required to balance the equation ... (note that '1's would not be shown in the equation)
a Ca(OH)_2(aq) + b HCl_(aq) ==> c CaCl_2(aq) + d H₂O_(l) ? [ab-38]
1. 1 2 1 1
2. 1 2 1 2
3. 2 1 1 2
4. 2 2 2 1
Which quantities a, b, c and d are required to balance the equation ... (note that '1's would not be shown in the equation)
a Al(OH)_3(s) + b HCl_(aq) ==> c AlCl_3(aq) + d H₂O_(l) ? [ab-39]
1. 2 6 2 3
2. 1 6 2 6
3. 1 3 1 3
4. 2 3 2 3
Which quantities a, b, c and d are required to balance the equation ... (note that '1's would not be shown in the equation)
a Fe₂O_3(s) + b HCl_(aq) ==> c FeCl_3(aq) + d H₂O_(l) ? [ab-40]
1. 2 6 2 3
2. 1 6 2 6
3. 1 3 1 3
4. 1 6 2 3
Which quantities a, b, c and d are required to balance the equation ... (note that '1's would not be shown in the equation)
a MgO_(s) + b HCl_(aq) ==> c MgCl_2(aq) + d H₂O_(l) ? [ab-41]
1. 1 2 1 1
2. 1 1 1 1
3. 2 2 1 2
4. 1 4 1 2
Which quantities a, b, c and d are required to balance the equation ... (note that '1's would not be shown in the equation)
a Mg(OH)_2(s) + b H₂SO_4(aq) ==> c MgSO_4(aq) + d H₂O_(l) ? [ab-42]
1. 1 2 1 1
2. 1 1 1 2
3. 2 2 1 2
4. 1 4 1 2
Which quantities a, b, c and d are required to balance the equation ... (note that '1's would not be shown in the equation)
a Li₂O_(s) + b HCl_(aq) ==> c LiCl_(aq) + d H₂O_(l) ? [ab-43]
1. 1 2 1 1
2. 1 1 1 1
3. 1 2 2 1
4. 1 2 1 2
Which quantities a, b, c and d are required to balance the equation ... (note that '1's would not be shown in the equation)
a KOH_(aq) + b H₂SO_4(aq) ==> c K₂SO_4(aq) + d H₂O_(l) ? [ab-44]
1. 1 2 1 1
2. 1 1 1 1
3. 2 2 1 2
4. 2 1 1 2
Which ions do acids always produce in water? [ab-45]
1. H⁺
2. OH^-
3. H₂⁺
4. O^2-
Which ions do alkalis always produce in water? [ab-46]
1. H⁺
2. OH^-
3. H₂⁺
4. O^2-
Which is the correct ionic equation for the neutralisation of an acid and an alkali? [ab-47]
1. 2H⁺_(aq) + O^2-_(aq) ==> 2H₂O_(l)
2. H^-_(aq) + OH⁺_(aq) ==> H₂O_(l)
3. H⁺_(aq) + OH^-_(aq) ==> H₂O_(l)
4. 4H⁺_(aq) + O^2-_(aq) ==> 2H₂O_(l)
When hydrochloric acid is neutralised with sodium hydroxide, which two ions have the highest concentrations in the resulting mixture? [ab-48]
1. H⁺ and OH^-
2. Na⁺ and OH^-
3. H⁺ and Cl^-
4. Na⁺ and Cl^-
Complete the symbol equation:
NH₃ + HCl ==> ...???... [ab-93]
1. NH₄Cl
2. NH₃HCl
3. NH₃Cl
4. NH₃
Complete the symbol equation:
NH₃ + HNO₃ ==> ...???... [ab-94]
1. NH₃HNO₃
2. NH₄NO₃
3. NH₃NO₃
4. NH₄HNO₃
Complete the symbol equation:
2NH₃ + H₂SO₄ ==> ...???... [ab-95]
1. (NH₃)₂HSO₄
2. NH₄₂SO₄
3. (NH₄)₂SO₄
4. NH₄HSO₄
Given the symbol equation:
MgO + 2HCl ==> ???? + H₂O
What is the missing ???? [ab-96]
1. MgCl
2. Mg₂Cl
3. 2MgCl
4. MgCl₂
Given the symbol equation:
Ca(OH)₂ + H₂SO₄ ==> CaSO₄ + ????
What is the missing ???? [ab-97]
1. 2H₂O
2. H₂O
3. 2H₂
4. H₂O₂
Given the symbol equation:
???? + 2HNO₃ ==> Zn(NO₃)₂ + H₂O + CO₂
What is the missing ???? [ab-98]
1. Zn(OH)₂
2. ZnCO₃
3. ZnHCO₃
4. ZnCO₂
Given the symbol equation:
Fe + H₂SO₄ ==> FeSO₄ + ????
What is the missing ???? [ab-99]
1. H₂O
2. HO₂
3. H₂
4. 2H₂
Given the symbol equation:
Na₂CO₃ + 2HCl ==> ???? + H₂O + CO₂
What is the missing ???? [ab-100]
1. NaCl
2. Na₂Cl₂
3. NaCl
4. 2NaCl
The equation shows the formation of sodium sulfate when sodium hydroxide neutralises sulfuric acid ....
H2SO4 + 2NaOH ==> Na2SO4 + 2H2O
An acid salt called sodium hydrogensulfate can also be made ...
H2SO4 + NaOH ==> NaHSO4 + H2O
50 cm3 of a sulfuric acid solution was neutralised by 20 cm3 of a sodium hydroxide solution to make sodium sulfate. What volume of sodium hydroxide solution is needed to form sodium hydrogensulfate from the 50cm3 of sulfuric acid? [ab-115]
1. 10 cm3
2. 15 cm3
3. 20 cm3
4. 25 cm3
The equation shows the formation of sodium sulfate when sodium hydroxide neutralises sulfuric acid ....
H2SO4 + 2NaOH ==> Na2SO4 + 2H2O
An acid salt called sodium hydrogensulfate can also be made ...
H2SO4 + NaOH ==> NaHSO4 + H2O
100 cm3 of a sulfuric acid solution was neutralised by 40 cm3 of a sodium hydroxide solution to make sodium sulfate. What volume of sodium hydroxide solution is needed to form sodium hydrogensulfate from the 100cm3 of sulfuric acid? [ab-116]
1. 10 cm3
2. 20 cm3
3. 50 cm3
4. 200 cm3
The equation shows the formation of sodium sulfate when sodium hydroxide neutralises sulfuric acid ....
H2SO4 + 2NaOH ==> Na2SO4 + 2H2O
An acid salt called sodium hydrogensulfate can also be made ...
H2SO4 + NaOH ==> NaHSO4 + H2O
70 cm3 of a sulfuric acid solution was neutralised by 15 cm3 of a sodium hydroxide solution to make sodium hydrogensulfate. What volume of sodium hydroxide solution is needed to form sodium sulfate from the 70cm3 of sulfuric acid? [ab-117]
1. 35 cm3
2. 20 cm3
3. 30 cm3
4. 40 cm3
The equation shows the formation of sodium sulfate when sodium hydroxide neutralises sulfuric acid ....
H2SO4 + 2NaOH ==> Na2SO4 + 2H2O
An acid salt called sodium hydrogensulfate can also be made ...
H2SO4 + NaOH ==> NaHSO4 + H2O
80 cm3 of a sulfuric acid solution was neutralised by 25 cm3 of a sodium hydroxide solution to make sodium hydrogensulfate. What volume of sodium hydroxide solution is needed to form sodium sulfate from the 80cm3 of sulfuric acid? [ab-118]
1. 40 cm3
2. 20 cm3
3. 25 cm3
4. 50 cm3
Method 1 (left)
Method 2 (above)
The diagrams show two ways of making a salt. Method 1 cannot be used for making transition metal salts because transition metal oxides or hydroxides are ..?.. [ab-119]
1. insoluble in water
2. too coloured to follow the reaction
3. unreactive with acids
4. not bases
Which of the following statements about acids and alkalis is TRUE? [ab-120]
1. hydrogen ions make sodium hydroxide solution alkaline
2. ammonium hydroxide is alkaline due to the presence of OH- ions
3. sulfuric acid is acid because it contains H- ions
4. hydrochloric acid solution is acidic because it contains hydroxide ions
Which of the following statements about acids and alkalis is TRUE? [ab-121]
1. hydrogen ions make sodium hydroxide solution alkaline
2. ammonium hydroxide is alkaline due to the presence of OH+ ions
3. sulfuric acid is acid because it contains H+ ions
4. hydrochloric acid solution is acidic because it contains hydroxide ions
Which of the following statements about acids and alkalis is TRUE? [ab-122]
1. the presence of oxide ions make sodium hydroxide solution alkaline
2. ammonium hydroxide is alkaline due to the presence of OH+ ions
3. sulfuric acid is acid because it contains H- ions
4. hydrochloric acid solution is acidic because it contains hydrogen ions
Which of the following statements about acids and alkalis is TRUE? [ab-123]
1. hydroxide ions make sodium hydroxide solution alkaline
2. ammonium hydroxide is alkaline due to the presence of OH+ ions
3. sulfuric acid is acid because it contains H- ions
4. hydrochloric acid solution is acidic because it contains hydride ions
What word specifically means 'a soluble base'? [ab-124]
1. acid
2. alkali
3. salt
4. dissolves
A molecule of hydrobromic acid (HBr) has one hydrogen that can be replaced by a metal to form a salt. Some acids have two hydrogens that can be replaced. If both hydrogens are replaced the 'normal' salt is formed. If one hydrogen only is replaced, an 'acid' salt is formed. Which of the following can form an acid salt? [ab-125]
1. nitric acid, HNO3
2. hydrochloric acid, HCl
3. carbonic acid, H2CO3
4. hydroiodic acid, HI
A molecule of hydrobromic acid (HBr) has one hydrogen that can be replaced by a metal to form a salt. Some acids have two hydrogens that can be replaced. If both hydrogens are replaced the 'normal' salt is formed. If one hydrogen only is replaced, an 'acid' salt is formed. Which of the following can form an acid salt? [ab-126]
1. nitric acid, HNO3
2. hydrochloric acid, HCl
3. hydroiodic acid, HI
4. sulfuric acid, H2SO4
When hydrochloric acid is neutralised with sodium hydroxide, which two ions have the lowest concentrations in the resulting mixture? [ab-127]
1. H⁺ and OH^-
2. Na⁺ and OH^-
3. H⁺ and Cl^-
4. Na⁺ and Cl^-
In the electrolysis of moderately concentrated sodium chloride solution (brine) using carbon/platinum electrodes, the principal product formed at the positive anode is? [ef1]
1. chlorine
2. hydrogen
3. oxygen
4. sodium
In the electrolysis of moderately concentrated sodium chloride solution (brine) using carbon/platinum electrodes, the principal product formed at the negative cathode is? [ef2]
1. chlorine
2. hydrogen
3. oxygen
4. sodium
When copper(II) sulfate solution undergoes electrolysis using carbon/platinum electrodes the product at the positive anode is? [ef3]
1. sulfur
2. hydrogen
3. oxygen
4. copper
When copper(II) sulfate solution undergoes electrolysis using carbon/platinum electrodes the product at the negative cathode is? [ef4]
1. sulfur
2. hydrogen
3. oxygen
4. copper
In the electrolysis of sodium sulfate solution with carbon/platinum electrodes, what product is formed on the surface of the negative cathode? [ef5]
1. hydrogen
2. oxygen
3. sodium
4. sulfur dioxide
In the electrolysis of sodium sulfate solution with carbon/platinum electrodes, what product is formed on the surface of the positive anode? [ef6]
1. hydrogen
2. oxygen
3. sodium
4. sulfur dioxide
In the electrolysis of water acidified with sulfuric acid, using carbon/platinum electrodes, what product is formed on the surface of the negative cathode? [ef7]
1. sulfur
2. sulfur dioxide
3. hydrogen
4. oxygen
In the electrolysis of water acidified with sulfuric acid, using carbon/platinum electrodes, what product is formed on the surface of the positive anode? [ef8]
1. copper ions
2. sulfur dioxide
3. hydrogen
4. oxygen
When copper(II) sulfate solution undergoes electrolysis using a carbon cathode and copper anode electrodes the product at the negative cathode is? [ef9]
1. copper
2. blue copper(II) ions
3. oxygen
4. hydrogen
When copper(II) sulfate solution undergoes electrolysis using a carbon cathode and copper anode electrodes the product at the positive anode is? [ef10]
1. copper
2. blue copper(II) ions
3. oxygen
4. hydrogen
When copper(II) chloride solution undergoes electrolysis using a carbon/platinum electrodes the product at the negative cathode is? [ef11]
1. hydrogen
2. blue copper(II) ions
3. copper
4. chlorine
When copper(II) chloride solution undergoes electrolysis using a carbon/platinum electrodes the product at the positive anode is? [ef12]
1. hydrogen
2. blue copper(II) ions
3. copper
4. chlorine
Which of the following statements is FALSE concerning the electrolysis of molten lead bromide, PbBr₂ ? [ef13]
1. solid lead bromide can also undergo electrolysis
2. lead is formed at the cathode
3. bromine is formed at the anode
4. molten lead bromide can be decomposed by the passage of a d.c. electric current
Which of the following statements is FALSE concerning the electrolysis of molten lead bromide, PbBr₂ ? [ef14]
1. solid lead bromide cannot undergo electrolysis
2. lead oxide is formed at the cathode
3. bromine is formed at the anode
4. molten lead bromide can be decomposed by the passage of a d.c. electric current
Which of the following statements is FALSE concerning the electrolysis of molten lead bromide, PbBr₂ ? [ef15]
1. solid lead bromide cannot undergo electrolysis
2. lead is formed at the cathode
3. oxygen is formed at the anode
4. molten lead bromide can be decomposed by the passage of a d.c. electric current
Which of the following statements is FALSE concerning the electrolysis of molten lead bromide, PbBr₂ ? [ef16]
1. solid lead bromide cannot undergo electrolysis
2. lead is formed at the cathode
3. bromine is formed at the anode
4. molten lead bromide can be decomposed by the passage of an a.c. electric current
Which of the following statements is FALSE concerning the electrolysis of molten sodium chloride, NaCl ? [ef17]
1. solid sodium chloride can also undergo electrolysis
2. sodium is formed at the cathode
3. chlorine is formed at the anode
4. molten sodium chloride can be decomposed by the passage of an d.c. electric current
Which of the following statements is FALSE concerning the electrolysis of molten sodium chloride, NaCl ? [ef18]
1. solid sodium chloride cannot undergo electrolysis
2. sodium is oxidised at the cathode
3. chlorine is formed at the anode
4. molten sodium chloride can be decomposed by the passage of an d.c. electric current
Which of the following statements is FALSE concerning the electrolysis of molten sodium chloride, NaCl ? [ef19]
1. solid sodium chloride cannot undergo electrolysis
2. sodium is formed at the cathode
3. chlorine is oxidised at the anode
4. molten sodium chloride can be decomposed by the passage of an d.c. electric current
Which of the following statements is FALSE concerning the electrolysis of molten sodium chloride, NaCl ? [ef20]
1. solid sodium chloride cannot undergo electrolysis
2. sodium is formed at the cathode
3. chlorine is formed at the anode
4. molten sodium chloride can be decomposed by the passage of an a.c. electric current
Which of the following statements is FALSE concerning the electrolysis of molten aluminium oxide, Al₂O₃ ? [ef21]
1. solid aluminium oxide can also undergo electrolysis
2. aluminium is formed at the cathode
3. oxygen is formed at the anode
4. molten aluminium oxide can be decomposed by the passage of an d.c. electric current
Which of the following statements is FALSE concerning the electrolysis of molten aluminium oxide, Al₂O₃ ? [ef22]
1. solid aluminium oxide cannot undergo electrolysis
2. aluminium is oxidised at the cathode
3. oxygen is formed at the anode
4. molten aluminium oxide can be decomposed by the passage of an d.c. electric current
Which of the following statements is FALSE concerning the electrolysis of molten aluminium oxide, Al₂O₃ ? [ef23]
1. solid aluminium oxide cannot undergo electrolysis
2. aluminium is formed at the cathode
3. oxygen cannot form at the anode
4. molten aluminium oxide can be decomposed by the passage of an d.c. electric current
Which of the following statements is FALSE concerning the electrolysis of molten aluminium oxide, Al₂O₃ ? [ef24]
1. solid aluminium oxide cannot undergo electrolysis
2. aluminium is formed at the cathode
3. oxygen is formed at the anode
4. molten aluminium oxide can be decomposed by the passage of an a.c. electric current
When copper(II) sulfate solution undergoes electrolysis using copper electrodes the product at the positive anode is? [ef25]
1. blue copper(II) ions
2. copper
3. hydrogen
4. oxygen
When copper(II) sulfate solution undergoes electrolysis using copper electrodes the product at the negative cathode is? [ef26]
1. blue copper(II) ions
2. copper
3. hydrogen
4. oxygen
Which of the following statements about electrolysis is FALSE? [ef27]
1. metals or hydrogen are formed at the cathode
2. any ionic compound dissolved in water can undergo electrolysis
3. an electrolyte is a solution or melt that cannot conduct a d.c. electrical current
4. positively charged ions migrate to the negatively charged cathode
Which of the following statements about electrolysis is FALSE? [ef28]
1. metals or hydrogen are formed at the cathode
2. any ionic compound dissolved in water can undergo electrolysis
3. an electrolyte is a solution or melt that contains ions and so conducts electricity
4. positively charged ions migrate to the anode
Which of the following statements about electrolysis is FALSE? [ef29]
1. metals or hydrogen are formed at the anode
2. any ionic compound dissolved in water can undergo electrolysis
3. an electrolyte is a solution or melt that contains ions and so conducts electricity
4. negatively charged ions migrate to the anode
Which of the following statements about electrolysis is FALSE? [ef30]
1. any ionic compound dissolved in water can undergo electrolysis
2. non-metals like oxygen and chlorine are formed at the cathode
3. an electrolyte is a solution or melt that contains ions and so conducts electricity
4. negatively charged ions migrate to the anode
Which of the following statements about electrolysis is FALSE? [ef31]
1. any ionic compound dissolved in water can undergo electrolysis
2. non-metals like oxygen and chlorine are formed at the anode
3. any compound dissolved in water can readily conduct electricity and undergo electrolysis.
4. positively charged ions migrate to the cathode
Which of the following statements about electrolysis is FALSE? [ef32]
1. any ionic compound dissolved in water can undergo electrolysis
2. non-metals like oxygen and chlorine are formed at the anode
3. solid ionic compounds cannot undergo electrolysis.
4. positively charged ions migrate to the anode
What do we call the positive electrode in an electrolysis cell? [ef33]
1. anode
2. cathode
3. electrolyte
4. anion
5. cation
What do we call the negative electrode in an electrolysis cell? [ef34]
1. anode
2. cathode
3. electrolyte
4. anion
5. cation
What do we call a negatively charged ion? [ef35]
1. anode
2. cathode
3. electrolyte
4. anion
5. cation
What do we call a positively charged ion? [ef36]
1. anode
2. cathode
3. electrolyte
4. anion
5. cation
Electrolysis is brought about by passing a d.c. electrical current through a solution of ions (electrolyte). Which of the following statements is FALSE? [eh-1]
1. oxidation involves electron gain
2. an electrolyte is an electrically conducting solution of ions
3. oxidation occurs at the anode
4. cations are reduced at an electrode
Electrolysis is brought about by passing a d.c. electrical current through a solution of ions (electrolyte). Which of the following statements is FALSE? [eh-2]
1. an electrolyte is an electrically conducting solution of ions
2. reduction involves electron loss
3. oxidation occurs at the anode
4. cations are reduced at an electrode
Electrolysis is brought about by passing a d.c. electrical current through a solution of ions (electrolyte). Which of the following statements is FALSE? [eh-3]
1. anions are oxidised at an electrode
2. reduction involves electron gain
3. oxidation occurs at the cathode
4. an electrolyte is an electrically conducting solution of ions
Electrolysis is brought about by passing a d.c. electrical current through a solution of ions (electrolyte). Which of the following statements is FALSE? [eh-4]
1. anions are oxidised at an electrode
2. reduction involves electron gain
3. an electrolyte is an electrically conducting solution of ions
4. cations are reduced at the anode
Given the following half-equation for what may happen on the surface of an electrode in electrolysis.
2H⁺(aq) + 2e^- ==> H₂(g)
Which statement is TRUE about this electrode equation? [eh-5]
1. it is a reduction at the cathode
2. it is an oxidation at the anode
3. the solution must to be acid for this cathode half-reaction to happen
4. it involves electron gain at the anode
Given the following half-equation for what may happen on the surface of an electrode in electrolysis.
2H⁺(aq) + 2e^- ==> H₂(g)
Which statement is TRUE about this electrode equation? [eh-6]
1. it is an oxidation at the anode
2. the solution does not have to be acid for this cathode half-reaction to happen
3. it is an oxidation at the cathode
4. it involves electron loss at the anode
Given the following half-equation for what may happen on the surface of an electrode in electrolysis.
2Cl^-(aq) ==> Cl₂(g) + 2e^-
Which statement is TRUE about this electrode equation? [eh-7]
1. it is a reduction at the cathode
2. it involves electron loss at the cathode
3. it is an oxidation at the anode
4. it involves electron gain at the anode
Given the following half-equation for what may happen on the surface of an electrode in electrolysis.
2Cl^-(aq) ==> Cl₂(g) + 2e^-
Which statement is TRUE about this electrode equation? [eh-8]
1. it is a reduction at the cathode
2. it involves electron loss at the cathode
3. it is a reduction at the anode
4. it involves electron loss at the anode
Given the following half-equation for what may happen on the surface of an electrode in electrolysis.
Cu²⁺(aq) + 2e^- ==> Cu(s)
Which statement is TRUE about this electrode equation? [eh-9]
1. it is a reduction at the cathode
2. it is an oxidation at the anode
3. it involves electron loss at the cathode
4. it involves electron gain at the anode
Given the following half-equation for what may happen on the surface of an electrode in electrolysis.
Cu²⁺(aq) + 2e^- ==> Cu(s)
Which statement is TRUE about this electrode equation? [eh-10]
1. it is an oxidation at the cathode
2. it involves electron gain at the cathode
3. it involves electron loss at the anode
4. it involves electron gain at the anode
Given the following half-equation for what may happen on the surface of an electrode in electrolysis.
Cu(s) ==> Cu²⁺(aq) + 2e^-
Which statement is TRUE about this electrode equation? [eh-11]
1. it is an oxidation at the cathode
2. it involves electron gain at the cathode
3. it involves electron loss at the anode
4. it involves reduction at the anode
Given the following half-equation for what may happen on the surface of an electrode in electrolysis.
Cu(s) ==> Cu²⁺(aq) + 2e^-
Which statement is TRUE about this electrode equation? [eh-12]
1. it is an oxidation at the cathode
2. it involves electron gain at the cathode
3. it involves electron gain at the anode
4. it involves an oxidation at the anode
Given the following half-equation for what may happen on the surface of an electrode in electrolysis.
4OH^- ==> 2H₂O(l) + O₂(g) + 4e^-
Which statement is TRUE about this electrode equation? [eh-13]
1. it involves electron loss at the anode
2. it involves electron gain at the cathode
3. it involves reduction at the anode
4. it involves an oxidation at the cathode
Given the following half-equation for what may happen on the surface of an electrode in electrolysis.
4OH^- ==> 2H₂O(l) + O₂(g) + 4e^-
Which statement is TRUE about this electrode equation? [eh-13]
1. it is an reduction at the cathode
2. it involves an oxidation at the anode
3. it involves electron gain at the anode
4. it involves electron loss at the cathode
Which of the following is the correctly balanced electrode half equation for the cathode in the electrolysis of acidified water? [eh-15]
1. 2H⁺(aq) + 2e^- ==> H₂(g)
2. 4OH^- ==> 2H₂O(l) + O₂(g) + 4e^-
3. H⁺(aq) + e^- ==> H(g)
4. 2OH^- ==> H₂O(l) + O₂(g) + 2e^-
Which of the following is the correctly balanced electrode half equation for the anode in the electrolysis of acidified water? [eh-16]
1. 2H⁺(aq) + 2e^- ==> H₂(g)
2. 4OH^- ==> 2H₂O(l) + O₂(g) + 4e^-
3. H⁺(aq) + e^- ==> H(g)
4. 2OH^- ==> H₂O(l) + O₂(g) + 2e^-
Which of the following is the correctly balanced electrode half equation for the cathode in the electrolysis of copper(II) sulfate with carbon electrodes? [eh-17]
1. Cu²⁺(aq) + 2e^- ==> Cu(s)
2. Cu(s) ==> Cu²⁺(aq) + 2e^-
3. 4OH^- ==> 2H₂O(l) + O₂(g) + 4e^-
4. 2OH^- ==> H₂O(l) + O₂(g) + 2e^-
5. Cu²⁺(aq) + e^- ==> Cu(s)
6. Cu(s) ==> Cu²⁺(aq) + e^-
Which of the following is the correctly balanced electrode half equation for the anode in the electrolysis of copper(II) sulfate with carbon electrodes? [eh-18]
1. Cu²⁺(aq) + 2e^- ==> Cu(s)
2. Cu(s) ==> Cu²⁺(aq) + 2e^-
3. 4OH^- ==> 2H₂O(l) + O₂(g) + 4e^-
4. 2OH^- ==> H₂O(l) + O₂(g) + 2e^-
5. Cu²⁺(aq) + e^- ==> Cu(s)
6. Cu(s) ==> Cu²⁺(aq) + e^-
Which of the following is the correctly balanced electrode half equation for the anode in the electrolysis of copper(II) sulfate with copper electrodes? [eh-19]
1. Cu²⁺(aq) + 2e^- ==> Cu(s)
2. Cu(s) ==> Cu²⁺(aq) + 2e^-
3. 4OH^- ==> 2H₂O(l) + O₂(g) + 4e^-
4. 2OH^- ==> H₂O(l) + O₂(g) + 2e^-
5. Cu²⁺(aq) + e^- ==> Cu(s)
6. Cu(s) ==> Cu²⁺(aq) + e^-
Which of the following is the correctly balanced electrode half equation for the cathode in the electrolysis of copper(II) sulfate with copper electrodes? [eh-20]
1. Cu²⁺(aq) + 2e^- ==> Cu(s)
2. Cu(s) ==> Cu²⁺(aq) + 2e^-
3. 4OH^- ==> 2H₂O(l) + O₂(g) + 4e^-
4. 2OH^- ==> H₂O(l) + O₂(g) + 2e^-
5. Cu²⁺(aq) + e^- ==> Cu(s)
6. Cu(s) ==> Cu²⁺(aq) + e^-

OCR GCSE 9-1 Gateway Science/Chemistry QUIZ on Topic C3 "CHEMICAL REACTIONS" (FT)

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