On-line chemical calculations Quiz for Higher GCSE (includes moles!)

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]
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]
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]
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]
Given the symbol equation to show the formation of iron sulphide:
Fe + S ==> FeS
Calculate the mass in g of iron sulphide formed when 5.6g of iron combines with 3.2g of sulphur.
(Relative atomic masses, A_r: Fe = 56 and S = 32) [com-5]
Given the symbol equation to show the formation of iron sulphide:
Fe + S ==> FeS
Calculate the mass in g of iron sulphide formed when 28g of iron combines with 16g of sulphur.
(Relative atomic masses, A_r: Fe = 56 and S = 32) [com-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 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]
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]
Given the symbol equation to show the formation of aluminium sulphide by heating a mixture of aluminium and sulphur:
2Al + 3S ==> Al₂S₃
How many g of sulphur is needed if 54g of aluminium is reacted to form 150g of aluminium sulphide?
(Relative atomic masses, A_r: Al = 27 and S = 32) [com-9]
Given the symbol equation to show the formation of aluminium sulphide by heating a mixture of aluminium and sulphur:
2Al + 3S ==> Al₂S₃
How many kg of sulphur is needed if 108kg of aluminium is reacted to form 300kg of aluminium sulphide?
(Relative atomic masses, A_r: Al = 27 and S = 32) [com-10]
Given the symbol equation to show the formation of iron sulphide by heating a mixture of iron and sulphur:
Fe + S ==> FeS
Calculate the mass in g of iron unreacted when 60g of iron reacts with 32g of sulphur to form 88g of iron sulphide.
(Relative atomic masses, A_r: Fe = 56 and S = 32) [com-11]
Given the symbol equation to show the formation of iron sulphide by heating a mixture of iron and sulphur:
Fe + S ==> FeS
Calculate the mass in g of sulphur unreacted when 28g of iron reacts with 22g of sulphur to form 44g of iron sulphide.
(Relative atomic masses, A_r: Fe = 56 and S = 32) [com-12]
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]
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]
Given the following relative atomic masses: Cu = 64, S = 32 and O = 16; calculate the relative formula mass of copper sulphate, CuSO₄ [rfm-1]
Given the following relative atomic masses: H = 1 and C = 12; calculate the relative molecular mass of ethane, C₂H₆ [rfm-2]
Given the following relative atomic masses: H = 1 and C = 12; calculate the relative molecular mass of octane, C₈H₁₈ [rfm-3]
Given the following relative atomic masses: H = 1, N = 14 and O = 16; calculate the relative formula mass of nitric acid, HNO₃ [rfm-4]
Given the following relative atomic masses: H = 1, N = 14 and O = 16; calculate the relative formula mass of ammonium nitrate, NH₄NO₃ [rfm-5]
Given the following relative atomic masses: H = 1, N = 14, O = 16 and S = 32; calculate the relative formula mass of ammonium sulphate, (NH₄)₂SO₄ [rfm-6]
Given the following relative atomic masses: H = 1, O = 16 and S = 32; calculate the relative formula mass of sulphuric acid, H₂SO₄ [rfm-7]
Given the following relative atomic masses: O = 16, Al = 27 and S = 32; calculate the relative formula mass of aluminium sulphate, Al₂(SO₄)₃ [rfm-8]
Given the following relative atomic masses: H = 1 and Cl = 35.5, calculate the relative formula mass of hydrochloric acid, HCl [rfm-9]
Given the following relative atomic masses: Na = 23 and Cl = 35.5, calculate the relative formula mass of sodium chloride, NaCl [rfm-10]
Given the following relative atomic masses: Ca = 40 and Cl = 35.5, calculate the relative formula mass of calcium chloride, CaCl₂ [rfm-11]
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]
Given the following relative atomic masses: Al = 27 and Cl = 35.5, calculate the relative formula mass of aluminium chloride, AlCl₃ [rfm-13]
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]
Given the following relative atomic masses: H = 1, C = 12 and O = 16; calculate the relative molecular mass of glucose, C₆H₁₂O₆ [rfm-5]
Given the following relative atomic masses: H = 1, C = 12 and O = 16; calculate the relative molecular mass of ethanol ('alcohol'), C₂H₅OH [rfm-16]
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]
Given the following relative atomic masses: O = 16 and Fe = 56; calculate the relative formula mass of iron(II) oxide, FeO [rfm-18]
Given the following relative atomic masses: O = 16 and Fe = 56; calculate the relative formula mass of iron(III) oxide, Fe₂O₃ [rfm-19]
Given the following relative atomic masses: O = 16 and Fe = 56; calculate the relative formula mass of the iron oxide, Fe₃O₄ [rfm-20]
Given the following relative atomic masses: H = 1 and C = 12; calculate the relative molecular mass of methane, CH₄ [rfm-21]
Given the following relative atomic masses: H = 1 and C = 12; calculate the relative molecular mass of propane, C₃H₈ [rfm-22]
Given the following relative atomic masses: C = 12 and O = 16; calculate the relative molecular mass of carbon dioxide, CO₂ [rfm-23]
Given the following relative atomic masses: C = 12, O = 16 and Cu = 64; calculate the relative formula mass of copper carbonate, CuCO₃ [rfm-23]
Given the following relative atomic masses: C = 12, O = 16 and Ca = 40; calculate the relative formula mass of calcium carbonate, CaCO₃ [rfm-23]
Given the atomic masses: Cu = 64, S = 32 and O = 16; calculate the % by mass of copper in copper(II) sulphate, CuSO₄ [pbm-1]
Given the atomic masses: H = 1 and C = 12; calculate the % by mass of carbon in ethane, C₂H₆ [pbm-2]
Given the atomic masses: H = 1 and C = 12; calculate the % by mass of carbon in octane, C₈H₁₈ [pbm-3]
Given the atomic masses: H = 1, N = 14 and O = 16; calculate the % by mass of hydrogen in nitric acid, HNO₃ [pbm-4]
Given the atomic masses: H = 1, N = 14 and O = 16; calculate the % by mass of hydrogen in ammonium nitrate, NH₄NO₃ [pbm-5]
Given the atomic masses: H = 1, N = 14, O = 16 and S = 32; calculate the % by mass of nitrogen in ammonium sulphate, (NH₄)₂SO₄ [pbm-6]
Given the atomic masses: H = 1, O = 16 and S = 32; calculate the % by mass of hydrogen in sulphuric acid, H₂SO₄ [pbm-7]
Given the atomic masses: O = 16, Al = 27 and S = 32; calculate the % by mass of aluminium in aluminium sulphate, Al₂(SO₄)₃ [pbm-8]
Given the atomic masses: H = 1 and Cl = 35.5, calculate the % by mass of hydrogen in hydrogen chloride, HCl [pbm-9]
Given the atomic masses: Na = 23 and Cl = 35.5, calculate the % by mass of sodium in sodium chloride, NaCl [pbm-10]
Given the atomic masses: Ca = 40 and Cl = 35.5, calculate the % by mass of calcium in calcium chloride, CaCl₂ [pbm-11]
Given the atomic masses: H = 1, O = 16 and Mg = 24, calculate the % by mass of magnesium in magnesium hydroxide, Mg(OH)₂ [pbm-12]
Given the atomic masses: Al = 27 and Cl = 35.5, calculate the % by mass of aluminium in aluminium chloride, AlCl₃ [pbm-13]
Given the atomic masses: H = 1, O = 16 and Al = 27, calculate the % by mass of aluminium in aluminium hydroxide, Al(OH)₃ [pbm-14]
Given the atomic masses: H = 1, C = 12 and O = 16; calculate the % by mass of carbon in glucose, C₆H₁₂O₆ [pbm-15]
Given the atomic masses: H = 1, C = 12 and O = 16; calculate the % by mass of carbon in ethanol ('alcohol'), C₂H₅OH [pbm-16]
Given the atomic masses: O = 16 and Fe = 56; calculate the % by mass of iron in iron(II) oxide, FeO [pbm-17]
Given the atomic masses: O = 16 and Fe = 56; calculate the % by mass of oxygen in iron(II) oxide, FeO [pbm-18]
Given the atomic masses: O = 16 and Fe = 56; calculate the % by mass of iron in iron(III) oxide, Fe₂O₃ [pbm-19]
Given the atomic masses: O = 16 and Fe = 56; calculate the % by mass of iron in the iron oxide, Fe₃O₄ [pbm-20]
Given the atomic masses: H = 1 and C = 12; calculate the % by mass of carbon in methane, CH₄ [pbm-21]
Given the atomic masses: H = 1 and C = 12; calculate the % by mass of carbon in propane, C₃H₈ [pbm-22]
Given the atomic masses: C = 12 and O = 16; calculate the % by mass of oxygen in carbon dioxide, CO₂ [pbm-23]
Given the atomic masses: C = 12, O = 16 and Cu = 64; calculate % by mass of copper in copper carbonate, CuCO₃ [pbm-24]
Given the atomic masses: C = 12, O = 16 and Ca = 40; calculate the % by mass of calcium in calcium carbonate, CaCO₃ [pbm-25]
Given the atomic masses: Cu = 64, S = 32 and O = 16; calculate the % by mass of oxygen in copper(II) sulphate, CuSO₄ [pbm-26]
Given the atomic masses: Cu = 64, S = 32 and O = 16; calculate the % by mass of sulphur in copper(II) sulphate, CuSO₄ [pbm-27]
Given the atomic masses: H = 1 and C = 12; calculate the % by mass of hydrogen in ethane, C₂H₆ [pbm-28]
Given the atomic masses: H = 1 and C = 12; calculate the % by mass of hydrogen in octane, C₈H₁₈ [pbm-29]
Given the atomic masses: H = 1, N = 14 and O = 16; calculate the % by mass of oxygen in nitric acid, HNO₃ [pbm-30]
Given the atomic masses: H = 1, N = 14 and O = 16; calculate the % by mass of nitrogen in nitric acid, HNO₃ [pbm-31]
Given the atomic masses: H = 1, N = 14 and O = 16; calculate the % by mass of nitrogen in ammonium nitrate, NH₄NO₃ [pbm-32]
Given the atomic masses: H = 1, N = 14 and O = 16; calculate the % by mass of oxygen in ammonium nitrate, NH₄NO₃ [pbm-33]
Given the atomic masses: H = 1, N = 14, O = 16 and S = 32; calculate the % by mass of hydrogen in ammonium sulphate, (NH₄)₂SO₄ [pbm-34]
Given the atomic masses: H = 1, N = 14, O = 16 and S = 32; calculate the % by mass of sulphur in ammonium sulphate, (NH₄)₂SO₄ [pbm-35]
Given the atomic masses: H = 1, N = 14, O = 16 and S = 32; calculate the % by mass of oxygen in ammonium sulphate, (NH₄)₂SO₄ [pbm-36]
Given the atomic masses: H = 1, O = 16 and S = 32; calculate the % by mass of oxygen in sulphuric acid, H₂SO₄ [pbm-37]
Given the atomic masses: O = 16, Al = 27 and S = 32; calculate the % by mass of sulphur in aluminium sulphate, Al₂(SO₄)₃ [pbm-38]
Given the atomic masses: O = 16, Al = 27 and S = 32; calculate the % by mass of oxygen in aluminium sulphate, Al₂(SO₄)₃ [pbm-39]
Given the atomic masses: H = 1 and Cl = 35.5, calculate the % by mass of chlorine in hydrogen chloride, HCl [pbm-40]
Given the atomic masses: Na = 23 and Cl = 35.5, calculate the % by mass of chlorine in sodium chloride, NaCl [pbm-41]
Given the atomic masses: Ca = 40 and Cl = 35.5, calculate the % by mass of chlorine in calcium chloride, CaCl₂ [pbm-42]
Given the atomic masses: H = 1, O = 16 and Mg = 24, calculate the % by mass of oxygen in magnesium hydroxide, Mg(OH)₂ [pbm-43]
Given the atomic masses: Al = 27 and Cl = 35.5, calculate the % by mass of chlorine in aluminium chloride, AlCl₃ [pbm-44]
Given the atomic masses: H = 1, C = 12 and O = 16; calculate the % by mass of hydrogen in glucose, C₆H₁₂O₆ [pbm-45]
Given the atomic masses: H = 1, C = 12 and O = 16; calculate the % by mass of oxygen in glucose, C₆H₁₂O₆ [pbm-46]
Given the atomic masses: H = 1, C = 12 and O = 16; calculate the % by mass of hydrogen in ethanol ('alcohol'), C₂H₅OH [pbm-47]
Given the atomic masses: H = 1, C = 12 and O = 16; calculate the % by mass of oxygen in ethanol ('alcohol'), C₂H₅OH [pbm-48]
Given the atomic masses: O = 16 and Fe = 56; calculate the % by mass of oxygen in iron(III) oxide, Fe₂O₃ [pbm-49]
Given the atomic masses: H = 1 and C = 12; calculate the % by mass of hydrogen in methane, CH₄ [pbm-50]
Given the atomic masses: O = 16 and Fe = 56; calculate the % by mass of oxygen in the iron oxide, Fe₃O₄ [pbm-51]
Given the atomic masses: C = 12, O = 16 and Ca = 40; calculate the % by mass of carbon in calcium carbonate, CaCO₃ [pbm-52]
Given the atomic masses: C = 12, O = 16 and Ca = 40; calculate the % by mass of oxygen in calcium carbonate, CaCO₃ [pbm-53]
If 54g of aluminium combines with oxygen to form 102g of aluminium oxide, what is the formula of aluminium oxide? (Relative atomic masses: Al = 27 and O = 16) [emp-1]
In an experiment, 56g of iron combined with exactly 64g of sulphur. What is the formula of the iron sulphide formed? (Relative atomic masses: Fe = 56 and S = 32) [emp-2]
In an experiment, 21g of lithium combined with exactly 14g of nitrogen. Work out the formula of lithium nitride. (Relative atomic masses: Li = 7 and N = 14) [emp-3]
If 168g of iron combined with oxygen to form 232g of an iron oxide, work out the formula of the iron oxide. (Relative atomic masses: Fe = 56 and O = 16) [emp-4]
If 28g of silicon combined with oxygen to form 60g of silicon oxide, work out the formula of silicon oxide. (Relative atomic masses: Si = 28 and O = 16) [emp-5]
In an experiment, heating 128g of copper combined with exactly 32g of sulphur. Work out the formula of the copper sulphide formed. (Relative atomic masses: Cu = 64 and S = 32) [emp-6]
In an experiment, excess chlorine was passed over 24g of heated magnesium metal until all the metal had reacted. If 95g of white magnesium chloride solid was formed, work out the formula of magnesium chloride. (Relative atomic masses: Mg = 24 and Cl = 35.5) [emp-7]
In an experiment, excess chlorine was passed over 27g of heated aluminium metal until all the metal had reacted. If 133.5g of white aluminium chloride was formed work out the formula of aluminium chloride. (Relative atomic masses: Al = 27 and Cl = 35.5) [emp-8]
In an experiment, excess chlorine was passed over 28g of heated silicon until all of it had reacted. If 170g of liquid silicon chloride was formed work out the formula of silicon chloride. (Relative atomic masses: Si = 28 and Cl = 35.5) [emp-9]
In an experiment, excess chlorine was passed over 31g of hot phosphorus until all of it had reacted. If 208.5g of white phosphorus chloride was formed work out the formula of phosphorus chloride. (Relative atomic masses: P = 31 and Cl = 35.5) [emp-10]
If 8g of sulphur combines with 12g of oxygen, what is the formula of the sulphur oxide formed? (Relative atomic masses: S = 32 and O = 16) [emp-11]
If 16g of sulphur combines with 103.5g of lead, what is the formula of the lead sulphide formed? (Relative atomic masses: Pb = 207 and S = 32) [emp-12]
If 40g of calcium combines with 160g of bromine, what is the formula of calcium bromide? (Relative atomic masses: Ca = 40 and Br = 80) [emp-13]
78g of potassium combines with 160g of bromine. What is the simplest formula of potssium bromide? (Relative atomic masses: K = 39 and Br = 80) [emp-14]
48g of magnesium combines with 320g of bromine, what is the formula of magnesium bromide? (Relative atomic masses: Mg = 24 and Br = 80) [emp-15]
160g of calcium combines with 64g of oxygen, what is the formula of calcium oxide? (Relative atomic masses: Ca = 40 and O = 16) [emp-16]
What is the formula of the phosphorus oxide formed when 62g of phosphorus combines with 80g of oxygen? (Relative atomic masses: P = 31 and O = 16) [emp-17]
72g of magnesium combines with 48g of oxygen, what is the formula of magnesium oxide? (Relative atomic masses: Mg = 24 and O = 16) [emp-18]
46g of sodium combined with 16g of oxygen. What is the formula of the sodium oxide formed? (Relative atomic masses: Na = 23 and O = 6) [emp-19]
78g of potassium combined with 32g of sulphur. What is the formula of potassium sulphide formed? (Relative atomic masses: K = 39 and S = 32) [emp-20]
56g of iron combined with 240g of bromine. What is the formula of the iron bromide formed? (Relative atomic masses: Fe = 56 and Br = 80) [emp-21]
If 20.9g of bismuth combines with 24.0g of bromine, what is the formula of the bismuth bromide formed? (Relative atomic masses: Bi = 209 and Br = 80) [emp-22]
If 54g of aluminium combines with 96g of sulphur, what is the formula of aluminium sulphide? (Relative atomic masses: = and = ) [emp-23]
When 117g of potassium combines with 31g of phosphorus, what is the formula of the potassium phosphide formed? (Relative atomic masses: K = 39 and P = 31) [emp-24]
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]
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]
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]
Iron sulphide can be made by heating an iron and sulphur mixture.
Fe_(s) + S_(s) ==> FeS_(s)
Given the atomic masses: Fe = 56, S = 32, how many g of iron sulphide can be made from 14g of iron? [rmc-4]
Iron sulphide can be made by heating an iron and sulphur mixture.
Fe_(s) + S_(s) ==> FeS_(s)
Given the atomic masses: Fe = 56, S = 32, how many g of sulphur reacts with 224g of iron? [rmc-5]
Iron sulphide can be made by heating an iron and sulphur 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 sulphide? [rmc-6]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
The salt sodium sulphate, Na₂SO₄, can be made by neutralising sodium hydroxide with sulphuric 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 sulphate? [rmc-19]
The salt sodium sulphate, Na₂SO₄, can be made by neutralising sodium hydroxide with sulphuric 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 sulphuric acid is needed to make 7.1g of sodium sulphate? [rmc-20]
The salt sodium sulphate, Na₂SO₄, can be made by neutralising sodium hydroxide with sulphuric 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 sulphate is formed when 8g of sodium hydroxide reacts? [rmc-21]
The salt sodium sulphate, Na₂SO₄, can be made by neutralising sodium hydroxide with sulphuric 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 46g of sulphuric acid reacts? [rmc-22]
Copper(I) sulphide 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]
Copper(I) sulphide 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]
Copper(I) sulphide ore can be converted to copper by roasting in air:
Cu₂S_(s) + O_2(g) ==> 2Cu_(s) + SO_2(g)
How many tonnes of sulphur dioxide are produced for every 1280 tonnes of ore processed?
(Relative atomic masses: Cu = 64, S = 32, O = 16) [rmc-25]
Copper(I) sulphide 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]
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]
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]
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]
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]
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]
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]
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]
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]
Chlorine consists of 75% chlorine-35 and 25% chlorine-37. Calculate the A_r of chlorine to 3sf/1dp. [ram-1]
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]
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]
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]
Antimony (Sb) is 57.2% Sb-121 and 42.8% Sb-123. Calculate the A_r of Sb to 4sf/1dp. [ram-5]
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]
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]
Europium consists of 47.8% Eu-151 and 52.2% Eu-153. Calculate A_r(Eu) to 4sf/1dp. [ram-8]
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]
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]
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]
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]
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]
Rubidium consists of the stable isotopes: ⁸⁵Rb (72.2%) and ⁸⁷Rb (27.8%). Calculate A_r(Rb) to 3sf/1dp. [ram-14]
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]
How many moles of iron are there in 2.8g? (atomic mass Fe = 56) [mam-1]
How many moles of sulphur are there in 64g? (atomic mass S = 32) [mam-2]
How many moles of sodium are there in 115g? (atomic mass Na = 23) [mam-3]
How many moles of carbon are there in 3g? (atomic mass C = 12 ) [mam-4]
How many moles of zinc are there in 1.625g? (atomic mass Zn = 65) [mam-5]
How many moles of iodine are there in 12.7g of I₂? (atomic mass I = 127) [mam-6]
How many moles of chlorine are there in 213g of Cl₂? (atomic mass Cl = 35.5) [mam-7]
How many moles of bromine are there in 6.4g of Br₂? (atomic mass Br = 80) [mam-8]
How many moles of phosphorus are there in 24.8g of P₄? (atomic mass P = 31) [mam-9]
How many moles of oxygen are there in 128g of O₂? (atomic mass O = 16) [mam-10]
How many moles of water are there in 4.5g of H₂O? (atomic masses: H = 1, O = 16) [mam-11]
How many moles of methane are there in 112g of CH₄? (atomic masses: C = 12, H = 1) [mam-12]
How many moles of sodium sulphate are there in 7.1g of Na₂SO₄? (atomic masses: Na = 23, S = 32, O = 16) [mam-13]
How many moles of sulphuric acid are there in 2.45g of H₂SO₄? (atomic masses: H = 1, S = 32, O = 16) [mam-14]
How many moles of calcium hydroxide are there in 25.9g of Ca(OH)₂? (atomic masses: Ca = 40, O = 16, H = 1) [mam-15]
How many g are there in 1.5 moles of aluminium? (atomic mass Al = 27) [mam-16]
How many g are there in 0.02 moles of uranium? (atomic mass U = 238) [mam-17]
How many g are there in 0.65 moles of magnesium? (atomic mass Mg = 24) [mam-18]
How many g are there in 0.23 moles of silicon? (atomic mass Si = 28) [mam-19]
How many g are there in 7.3 moles of boron? (atomic mass B = 10.8) [mam-20]
How many g are there in 0.05 moles of nitrogen, N ₂? (atomic mass N = 14) [mam-21]
How many g are there in 0.75 moles of ozone, O₃? (atomic mass O = 16) [mam-22]
How many g are there in 2.5 moles of oxygen, O₂? (atomic mass O = 16) [mam-23]
How many g are there in 0.16 moles of chlorine, Cl₂? (atomic mass Cl = 35.5) [mam-24]
How many g are there in 1.65 moles of iodine, I₂? (atomic mass I = 127) [mam-25]
How many g are there in 3.6 moles of sodium hydroxide, NaOH? (atomic masses: Na = 23, O = 16, H = 1) [mam-26]
How many g are there in 1.5 moles of nitric acid, HNO₃? (atomic masses: H = 1, N = 14, O = 16) [mam-27]
How many g are there in 0.15 moles of ammonium sulphate, (NH₄)₂SO₄? (atomic masses: N = 14, H = 1, S = 32, O = 16) [mam-28]
How many g are there in 0.8 moles of aluminium hydroxide, Al(OH)₃? (atomic masses: Al = 27, O = 16, H = 1) [mam-29]
How many g are there in 0.005 moles of sodium thiosulphate, Na₂S₂O₃? (atomic masses: Na = 23, S = 32, O =16) [mam-30]
It was found that 0.2 moles of atoms of an element had a mass of 3.2g. What is the relative atomic mass of the element? [mam-31]
It was found that 0.005 moles of atoms of an element had a mass of 0.295g. What is the relative atomic mass of the element? [mam-32]
It was found that 0.15 moles of atoms of an element had a mass of 10.95g. What is the relative atomic mass of the element? [mam-33]
It was found that 0.4 moles of atoms of an element had a mass of 56.2g. What is the relative atomic mass of the element? [mam-34]
It was found that 0.015 moles of atoms of an element had a mass of 2.88g. What is the relative atomic mass of the element? [mam-35]
It was found that 0.25 moles of atoms of an element had a mass of 40.65g. What is the relative atomic mass of the element? [mam-36]
It was found that 0.002 moles of a compound had a mass of 0.24g. What is the relative formula mass of the compound? [mam-37]
It was found that 0.005 moles of a compound had a mass of 0.2025g. What is the relative formula mass of the compound? [mam-38]
It was found that 0.25 moles of a compound had a mass of 14.05g. What is the relative formula mass of the compound? [mam-39]
It was found that 0.025 moles of a compound had a mass of 0.70g. What is the relative formula mass of the compound? [mam-40]
0.55g of boron combined with 1.2g of oxygen. Deduce the empirical formula of boron oxide. (relative atomic masses, A_r: B = 11, O = 16) [efm-1]
1.35g of aluminium was burned in excess fluorine to form 4.2g of aluminium fluoride. Deduce the empirical formula of aluminium fluoride. (relative atomic masses, A_r: Al = 27, F = 19) [efm-2]
3.4g of an unusual carbon oxide contained 1.8g of carbon. Deduce the empirical formula of the carbon oxide. (relative atomic masses, A_r: C = 12, O = 16) [efm-3]
In an experiment 3.175g of copper combined with 0.400g of oxygen. What is the empirical formula of the copper oxide? (relative atomic masses, A_r: Cu = 63.5, O = 16) [efm-4]
8.875g of chlorine combined with 14.25g of fluorine. What is the formula of the chlorine fluoride? (relative atomic masses, A_r: Cl = 35.5, F = 19) [efm-5]
A gas formed by the combination of hydrogen and sulphur consited of 5.88% hydrogen and 94.12% sulphur. What is its empirical formula? (relative atomic masses, A_r: H = 1, S = 32) [efm-6]
5.08g of iodine combined with 1.6g of oxygen. What is the formula of the iodine oxide? (relative atomic masses, A_r: I = 127, O = 16) [efm-7]
2.8g of lithium was heated in a stream of air forming 6.0g of lithium oxide. What is its formula? (relative atomic masses, A_r: Li = 7, O =16) [efm-8]
A iron-copper sulphide ore consisted of 30.5% iron, 34.6% copper, and 34.9% sulphur. What is the empirical formula of the ore? (relative atomic masses, A_r: Fe = 56, Cu = 63.5, S = 32) [efm-9]
0.48g of magnesium combined with 3.20g of bromine. What is the formula of magnesium bromide? (relative atomic masses, A_r: Mg = 24, Br = 80) [efm-10]
0.7g of nitrogen combined with 5.325g of chlorine. Deduce the formula of nitrogen chloride. (relative atomic masses, A_r: N = 14, Cl = 35.5) [efm-11]
Fluorine oxide consists of 70.4% fluorine and 29.6% oxygen by mass. Deduce the formula of fluorine oxide. (relative atomic masses, A_r: F = 19, O = 16) [efm-12]
47.6g of uranium combined with 22.8g of fluorine. What is the empirical formula of this uranium fluoride? (relative atomic masses, A_r: U = 238, F = 19) [efm-13]
10.35g of lead was heated in excess oxygen. If 11.95g of a lead oxide was formed, deduce its empirical formula. (relative atomic masses, A_r: Pb = 207, O = 16) [efm-14]
10.8g of aluminium combined with 19.2g of sulphur. What is the empirical formula of aluminium sulphide? (relative atomic masses, A_r: Al = 27, S = 32) [efm-15]
A hydrocarbon of molecular mass 30 consisted of 80% carbon and 20% hydrogen by mass. Deduce the molecular formula of the hydrocarbon. (relative atomic masses, A_r: C = 12, H = 1) [efm-16]
6g of carbon combines with 71g of chlorine. What is the formula of the carbon chloride? (relative atomic masses, A_r: C = 12, Cl = 35.5) [efm-17]
An organic compound consisted of 52.18% carbon, 13.04% hydrogen and 34.78% oxygen by mass. Deduce its empirical formula. (relative atomic masses, A_r: C = 12, H = 1, O = 16) [efm-18]
An chlorinated hydrocabon molecule consisted of 37.21% carbon, 7.75% hydrogen and 55.04% chlorine by mass. Deduce its empirical formula. (relative atomic masses, A_r: C = 12, H = 1, Cl = 35.5) [efm-19]
A calcium mineral consisted of 29.4% calcium, 23.5% sulphur and 47.1% oxygen by mass. Calculate the empirical formula of the mineral. (relative atomic masses, A_r: Ca = 40, S = 32, O = 16) [efm-20]
A salt consisted of 27.06% sodium, 16.47% nitrogen and 56.47% oxygen by mass. Deduce the formula of the salt. (relative atomic masses, A_r: Na = 23, N = 14, O = 16) [efm-21]
A brominated hydrocarbon consisted of 12.77% carbon, 2.13% hydrogen and 85.10% bromine by mass. If its molecular mass is 188, deduce the molecular formula of the molecule. (relative atomic masses, A_r: C = 12, H = 1, Br =80) [efm-22]
It was found that 24g of carbon was combined with 5g of hydrogen in a hydrocarbon. If its molecular mass was 58, what is its molecular formula? (relative atomic masses, A_r: C = 12, H = 1) [efm-23]
A hydrocarbon consisted of 92.3% carbon and 7.7% hydrogen. If its molecular mass is 78, work out its molecular formula. (relative atomic masses, A_r: C = 12, H = 1) [efm-24]
A carbohydrate on analysis consisted of 40.00% carbon, 6.67% hydrogen and 53.33% oxygen. If its molecular mass is 180, deduce the molecular formula of the carbohydrate. (relative atomic masses, A_r: C = 12, H = 1, O = 16) [efm-25]
7.75g of an alcohol consisted of 3.00g carbon, 0.75g hydrogen and 4.00g oxygen. If its molecular mass is 62, work out the molecular formula. (relative atomic masses, A_r: C = 12, H = 1, O = 16) [efm-26]
An alcohol consisted of 39.13% carbon, 8.70% hydrogen and 52.17% oxygen. If its molecular mass is 92, deduce its molecular formula. (relative atomic masses, A_r: C = 12, H = 1, O = 16) [efm-27]
In an experiment 6g of carbon combined with 19g of fluorine. Calculate the molecular formula of the compound formed if the molecular mass of it is 100. (relative atomic masses, A_r: C = 12, F = 19) [efm-28]
A compound of hydrogen and oxygen was made up of 0.5g hydrogen and 8g of oxygen. What is its empirical formula? (relative atomic masses, A_r: H = 1, O = 16) [efm-29]
A lithium compound consisted of 7g of lithium combined with 16g of sulphur and 32g of oxgen. What is the empirical formula of the compound? (relative atomic masses, A_r: Li = 7, S = 32, O = 16) [efm-30]
58g of a sodium phosphate salt consisted of 34.5g of sodium, 15.5g of phosphorus and 32.0g of oxygen. What is the simplest formula of the compound? (relative atomic masses, A_r: Na = 23, P = 31, O = 16) [efm-31]
A sodium compound consisted of 46g of sodium combined with 254g of iodine and 128g of oxygen. What is the compounds empirical formula? (relative atomic masses, A_r: Na = 23, I = 127, O = 16) [efm-32]
16g of copper, after heating in oxygen, formed 20g of a copper oxide. What is the formula of the oxide? (relative atomic masses, A_r: Cu = 64, O = 16) [efm-33]
An oxide of carbon consisted of 3g of carbon combined with 4g of oxygen. What is the formula of the oxide? (relative atomic masses, A_r: C = 12, O = 16) [efm-34]
1.95g of potassium combined with 4.00g of bromine. What is the empirical formula of the compound? (relative atomic masses, A_r: K = 39, Br = 80) [efm-35]
5g of calcium on heating in oxygen formed 7g of calcium oxide. What is the simplest formula of calcium oxide? (relative atomic masses, A_r: Ca = 40, O = 16) [efm-36]
13g of zinc combined with 6.4g of sulphur. What is the empirical formula of zinc sulphide? (relative atomic masses, A_r: Zn = 65, S = 32) [efm-37]
An oxide of copper contained 80% copper and 20% oxygen by mass. What is the formula of the copper oxide? (relative atomic masses, A_r: Cu = 64, O = 16) [efm-38]
If magnesium oxide consists of 60% magnesium and 40% oxygen, what is its simplest formula? (relative atomic masses, A_r: Mg = 24, O = 16) [efm-39]
2.3g of sodium combined with 1.6g of sulphur. What is the formula of sodium sulphide? (relative atomic masses, A_r: Na = 23, S = 32) [efm-40]
In an experiment 1.28g of copper combined with 0.16g of oxygen. What is the formula of the copper oxide? (relative atomic masses, A_r: Cu = 64, O = 16) [efm-41]
13.8g of sodium combined with 6.2g of phosphorus. What is the formula of sodium phosphide? (relative atomic masses, A_r: Na = 23, P = 31) [efm-42]
10g of calcium combined with 40g of bromine. What is the formula of calcium bromide? (relative atomic masses, A_r: Ca = 40, Br = 80) [efm-43]
22g of boron combined with 114g of fluorine. What is the empirical formula of boron fluoride? (relative atomic masses, A_r: B = 11, F = 19) [efm-44]
1.2g of titanium, after heating in oxygen, formed 2.0g of a titanium oxide. What is the empirical formula for the titanium oxide? (relative atomic masses, A_r: Ti = 48, O = 16) [efm-45]
0.800g of magnesium reacted with 8.467g of iodine. Calculate the empirical formula for magnesium iodide.? (relative atomic masses, A_r: Mg = 24, I = 127) [efm-46]
Given the equation: 2Na_(s) + 2H₂O_(l) ==> 2NaOH_(aq) + H_2(g)
Calculate the volume of hydrogen formed in dm³ when 2.3g of sodium reacts with water. (A_r's Na=23, H=1, O=16, 1 mol gas = 24 dm³ at room temp./press.) [mvg-1]
Given the equation: 2Na_(s) + 2H₂O_(l) ==> 2NaOH_(aq) + H_2(g)
Calculate the volume of hydrogen formed in dm³ when 9.2g of sodium reacts with water. (A_r's Na=23, H=1, O=16, 1 mol gas = 24 dm³ at room temp./press.) [mvg-2]
Given the equation: 2Na_(s) + 2H₂O_(l) ==> 2NaOH_(aq) + H_2(g)
What mass of sodium in g will form 600 cm³ of hydrogen gas? (A_r's Na=23, H=1, O=16, 1 mol gas = 24 dm³ at room temp./press.) [mvg-3]
Given the equation: 2Na_(s) + 2H₂O_(l) ==> 2NaOH_(aq) + H_2(g)
What mass of sodium in g will form 18 dm³ of hydrogen gas? (A_r's Na=23, H=1, O=16, 1 mol gas = 24 dm³ at room temp./press.) [mvg-4]
Given the equation for the thermal decomposition of calcium carbonate (limestone):
CaCO_3(s) ==> CaO_(s) + CO_2(g)
What volume of carbon dioxide in dm³ is formed when 10g of limestone is heated strongly? (A_r's Ca=40, C=12, O=16, 1 mol gas = 24 dm³ at room temp./press.) [mvg-5]
Given the equation for the thermal decomposition of calcium carbonate (limestone):
CaCO_3(s) ==> CaO_(s) + CO_2(g)
What volume of carbon dioxide in dm³ is formed when 200g of limestone is heated strongly? (A_r's Ca=40, C=12, O=16, 1 mol gas = 24 dm³ at room temp./press.) [mvg-6]
Given the equation for the thermal decomposition of calcium carbonate (limestone):
CaCO_3(s) ==> CaO_(s) + CO_2(g)
What mass of limestone in g, on strong heating, will form 6 dm³ carbon dioxide? (A_r's Ca=40, C=12, O=16, 1 mol gas = 24 dm³ at room temp./press.) [mvg-7]
Given the equation for the thermal decomposition of calcium carbonate (limestone):
CaCO_3(s) ==> CaO_(s) + CO_2(g)
What mass of limestone in g, on strong heating, will form 120 cm³ carbon dioxide? (A_r's Ca=40, C=12, O=16, 1 mol gas = 24 dm³ at room temp./press.) [mvg-8]
5 g of a gas had a volume of 60 dm³. What is its molecular mass? (1 mol gas = 24 dm³ at room temp./press.) [mvg-9]
What is the volume in dm³ of 8 g of a gas of molecular mass 16? (1 mol gas = 24 dm³ at room temp./press.) [mvg-10]
What mass of gas, of molecular mass 36.5, is present in 4.8 dm³ of the gas? (1 mol gas = 24 dm³ at room temp./press.) [mvg-11]
0.145 g of a gas had a volume of 60 cm³. What is its molecular mass? (1 mol gas = 24 dm³ at room temp./press.) [mvg-12]
What is the volume in dm³ of 0.85 g of a gas of molecular mass 17? (1 mol gas = 24 dm³ at room temp./press.) [mvg-13]
What mass of gas, of molecular mass 71, is present in 1.2 dm³ of the gas? (1 mol gas = 24 dm³ at room temp./press.) [mvg-14]
2.55g of a gas had a volume of 0.6 dm³. What is its molecular mass? (1 mol gas = 24 dm³ at room temp./press.) [mvg-15]
What is the volume in dm³ of 1 g of a gas of molecular mass 96? (1 mol gas = 24 dm³ at room temp./press.) [mvg-16]
What mass of gas, of molecular mass 44, is present in 0.15 dm³ of the gas? (1 mol gas = 24 dm³ at room temp./press.) [mvg-17]
What is the volume in dm³ of 0.8 g of a gas of molecular mass 32? (1 mol gas = 24 dm³ at room temp./press.) [mvg-18]
Given the equation for magnesium dissolving in hydrochloric acid:
Mg_(s) + 2HCl_(aq) ==> MgCl_2(aq) + H_2(g)
What mass of magnesium in g, will form 1.2 dm³ of hydrogen gas? (A_r's Mg=24, H=1, Cl=35.5, 1 mol gas = 24 dm³ at room temp./press.) [mvg-19]
Given the equation for magnesium dissolving in hydrochloric acid:
Mg_(s) + 2HCl_(aq) ==> MgCl_2(aq) + H_2(g)
What mass of magnesium in g, will form 36 dm³ of hydrogen gas? (A_r's Mg=24, H=1, Cl=35.5, 1 mol gas = 24 dm³ at room temp./press.) [mvg-20]
Given the equation for magnesium dissolving in hydrochloric acid:
Mg_(s) + 2HCl_(aq) ==> MgCl_2(aq) + H_2(g)
What volume of hydrogen gas, in dm³, is formed when 4g of magnesium dissolves in the acid? (A_r's Mg=24, H=1, Cl=35.5, 1 mol gas = 24 dm³ at room temp./press.) [mvg-21]
Given the equation for magnesium dissolving in hydrochloric acid:
Mg_(s) + 2HCl_(aq) ==> MgCl_2(aq) + H_2(g)
What volume of hydrogen gas, in dm³, is formed when 72g of magnesium dissolves in the acid? (A_r's Mg=24, H=1, Cl=35.5, 1 mol gas = 24 dm³ at room temp./press.) [mvg-22]
Given the equation for aluminium dissolving in dilute sulphuric acid:
2Al_(s) + 3H₂SO_4(aq) ==> Al₂(SO₄)_3(aq) + 3H_2(g)
What mass of aluminium in g, dissolves when 7.2 dm³ of hydrogen is formed? (A_r's: Al=27, H=1, S=32, O=16, 1 mol gas = 24 dm³ at room temp./press.) [mvg-23]
Given the equation for aluminium dissolving in dilute sulphuric acid:
2Al_(s) + 3H₂SO_4(aq) ==> Al₂(SO₄)_3(aq) + 3H_2(g)
What mass of aluminium in g, dissolves when 48 dm³ of hydrogen is formed? (A_r's: Al=27, H=1, S=32, O=16, 1 mol gas = 24 dm³ at room temp./press.) [mvg-24]
Given the equation for aluminium dissolving in dilute sulphuric acid:
2Al_(s) + 3H₂SO_4(aq) ==> Al₂(SO₄)_3(aq) + 3H_2(g)
What volume of hydrogen, in dm³, is formed, when 54g of aluminium dissolves? (A_r's: Al=27, H=1, S=32, O=16, 1 mol gas = 24 dm³ at room temp./press.) [mvg-25]
Given the equation for aluminium dissolving in dilute sulphuric acid:
2Al_(s) + 3H₂SO_4(aq) ==> Al₂(SO₄)_3(aq) + 3H_2(g)
What volume of hydrogen, in dm³, when 27g of aluminium dissolves? (A_r's: Al=27, H=1, S=32, O=16, 1 mol gas = 24 dm³ at room temp./press.) [mvg-26]
Given the equation for calcium carbonate dissolving in hydrochloric acid:
CaCO_3(s) + 2HCl_(aq) ==> CaCl_2(aq) H₂O_(l) + CO_2(g)
Calculate the volume of carbon dioxide, in dm³, when 5 g of calcium carbonate dissolves in the acid. (A_r's: Ca=40, C=12, O=16, Cl=35.5, 1 mol gas = 24 dm³ at room temp./press.) [mvg-27]
Given the equation for calcium carbonate dissolving in hydrochloric acid:
CaCO_3(s) + 2HCl_(aq) ==> CaCl_2(aq) H₂O_(l) + CO_2(g)
Calculate the volume of carbon dioxide, in dm³, when 400 g of calcium carbonate dissolves in the acid. (A_r's: Ca=40, C=12, O=16, Cl=35.5, 1 mol gas = 24 dm³ at room temp./press.) [mvg-28]
Given the equation for calcium carbonate dissolving in hydrochloric acid:
CaCO_3(s) + 2HCl_(aq) ==> CaCl_2(aq) H₂O_(l) + CO_2(g)
Calculate the mass of calcium carbonate (in g) that dissolves when 6 dm³ of carbon dioxide is formed. (A_r's: Ca=40, C=12, O=16, Cl=35.5, 1 mol gas = 24 dm³ at room temp./press.) [mvg-29]
Given the equation for calcium carbonate dissolving in hydrochloric acid:
CaCO_3(s) + 2HCl_(aq) ==> CaCl_2(aq) H₂O_(l) + CO_2(g)
Calculate the mass of calcium carbonate (in g) that dissolves when 36 dm³ of carbon dioxide is formed. (A_r's: Ca=40, C=12, O=16, Cl=35.5, 1 mol gas = 24 dm³ at room temp./press.) [mvg-30]
Given the reaction between hydrogen and chlorine to form hydrogen chloride:
H_2(g) + Cl_2(g) ==> 2HCl_(g)
What volume of hydrogen in cm³ is needed to make 100cm³ of hydrogen chloride? [rgv-1]
Given the reaction between hydrogen and chlorine to form hydrogen chloride:
H_2(g) + Cl_2(g) ==> 2HCl_(g)
What volume of chlorine in dm³ is needed to make 40dm³ of hydrogen chloride? [rgv-2]
Given the reaction between hydrogen and chlorine to form hydrogen chloride:
H_2(g) + Cl_2(g) ==> 2HCl_(g)
What volume of hydrogen chloride in dm³ is made by reacting 20dm³ of hydrogen? [rgv-3]
Given the reaction between hydrogen and chlorine to form hydrogen chloride:
H_2(g) + Cl_2(g) ==> 2HCl_(g)
What volume of hydrogen chloride in cm³ is made by reacting 300cm³ of chlorine? [rgv-4]
Given the reaction between nitrogen and hydrogen to form ammonia:
N_2(g) + 3H_2(g) ==> 2NH_3(g)
What volume of ammonia in cm³ is formed if 180cm³ of hydrogen reacts? [rgv-5]
Given the reaction between nitrogen and hydrogen to form ammonia:
N_2(g) + 3H_2(g) ==> 2NH_3(g)
What volume of ammonia in dm³ is formed if 40dm³ of nitrogen reacts? [rgv-6]
Given the reaction between nitrogen and hydrogen to form ammonia:
N_2(g) + 3H_2(g) ==> 2NH_3(g)
What volume of hydrogen in dm³ is needed to make 60dm³ of ammonia? [rgv-7]
Given the reaction between nitrogen and hydrogen to form ammonia:
N_2(g) + 3H_2(g) ==> 2NH_3(g)
What volume of nitrogen in cm³ is needed to make 640cm³ of ammonia? [rgv-8]
The combustion of methane is given by the equation:
CH_4(g) + 2O_2(g) ==> CO_2(g) + 2H₂O_(l)
What volume of oxygen in cm³ is needed to burn 200cm³ of methane? [rgv-9]
The combustion of methane is given by the equation:
CH_4(g) + 2O_2(g) ==> CO_2(g) + 2H₂O_(l)
What volume of carbon dioxide in cm³ is formed on burning 10cm³ of methane? [rgv-10]
The combustion of methane is given by the equation:
CH_4(g) + 2O_2(g) ==> CO_2(g) + 2H₂O_(g)
What is the total volume of gases produced in cm³ when 30cm³ of methane burns? [rgv-11]
The combustion of propane is given by the equation:
C₃H_8(g) + 5O_2(g) ==> 3CO_2(g) + 4H₂O_(l)
What volume of oxygen in cm³ is needed to burn 20cm³ of propane? [rgv-12]
The combustion of propane is given by the equation:
C₃H_8(g) + 5O_2(g) ==> 3CO_2(g) + 4H₂O_(l)
What volume of propane in cm³ can be completely burned by 200cm³ of oxygen? [rgv-13]
The combustion of propane is given by the equation:
C₃H_8(g) + 5O_2(g) ==> 3CO_2(g) + 4H₂O_(l)
What volume of carbon dioxide in dm³ is formed by burning 30dm³ of propane? [rgv-14]
The combustion of propane is given by the equation:
C₃H_8(g) + 5O_2(g) ==> 3CO_2(g) + 4H₂O_(g)
What total volume of gases in cm³ is formed by burning 40cm³ of propane? [rgv-15]
The combustion of propane is given by the equation:
C₃H_8(g) + 5O_2(g) ==> 3CO_2(g) + 4H₂O_(g)
What volume of steam in cm³ is formed by burning 20cm³ of propane? [rgv-16]
The combustion of ethane is given by the equation:
2C₂H_6(g) + 7O_2(g) ==> 4CO_2(g) + 6H₂O_(l)
What volume of carbon dioxide in cm³ is formed by burning 20cm³ of ethane? [rgv-17]
The combustion of ethane is given by the equation:
2C₂H_6(g) + 7O_2(g) ==> 4CO_2(g) + 6H₂O_(l)
What volume of oxygen in cm³ is needed to completely burn 60cm³ of ethane? [rgv-18]
The combustion of ethane is given by the equation:
2C₂H_6(g) + 7O_2(g) ==> 4CO_2(g) + 6H₂O_(g)
What volume of steam in dm³ is formed when 40dm³ of ethane burns? [rgv-19]
The combustion of ethane is given by the equation:
2C₂H_6(g) + 7O_2(g) ==> 4CO_2(g) + 6H₂O_(g)
What total volume of gases in dm³ are formed when 15dm³ of ethane burns? [rgv-20]
The combustion of ethane is given by the equation:
2C₂H_6(g) + 7O_2(g) ==> 4CO_2(g) + 6H₂O_(g)
What volume of ethane in cm³ can be burned completely using 175cm³ of oxygen? [rgv-21]
A cracking reaction to break down a large hydrocarbon molecule into, in order, hexane, propene and ethene, is shown below.
C₁₈H_38(g) ==> C₆H_14(g) + 2C₃H_6(g) + 3C₂H_4(g)
What total volume in dm³ of hydrocarbon gases are formed when 20dm³ of the large hydrocarbon are broken down? [rgv-22]
A cracking reaction to break down a large hydrocarbon molecule into, in order, hexane, propene and ethene, is shown below.
C₁₈H_38(g) ==> C₆H_14(g) + 2C₃H_6(g) + 3C₂H_4(g)
What volume in cm³ of propene gas is formed when 120cm³ of the large hydrocarbon are broken down? [rgv-23]
A cracking reaction to break down a large hydrocarbon molecule into, in order, hexane, propene and ethene, is shown below.
C₁₈H_38(g) ==> C₆H_14(g) + 2C₃H_6(g) + 3C₂H_4(g)
What volume in cm³ of ethene gas is formed when 40cm³ of the large hydrocarbon are broken down? [rgv-24]
What is the molarity of the solution formed by dissolving 20 g of sodium hydroxide (NaOH) in 1000 cm³ of water? (A_r's: Na=23, O=16, H=1) [msc-1]
What is the molarity of the solution formed by dissolving 10 g of sodium hydroxide (NaOH) in 500 cm³ of water? (A_r's: Na=23, O=16, H=1) [msc-2]
What is the molarity of the solution formed by dissolving 80 g of sodium hydroxide (NaOH) in 500 cm³ of water? (A_r's: Na=23, O=16, H=1) [msc-3]
What is the molarity of the solution formed by dissolving 9.8 g of sulphuric acid (H₂SO₄) in 1000 cm³ of water? (A_r's: H=1, S=32, O=16) [msc-4]
What is the molarity of the solution formed by dissolving 196 g of sulphuric acid (H₂SO₄) in 1000 cm³ of water? (A_r's: H=1, S=32, O=16) [msc-5]
What is the molarity of the solution formed by dissolving 49 g of sulphuric acid (H₂SO₄) in 250 cm³ of water? (A_r's: H=1, S=32, O=16) [msc-6]
What mass (g) of potassium hydroxide (KOH) is needed to make up 1000cm³ of a solution of concentration 1mol/dm³? (A_r's: K=39, O=16, H=1) [msc-7]
What mass (g) of potassium hydroxide (KOH) is needed to make up 500cm³ of a solution of concentration 0.2mol/dm³? (A_r's: K=39, O=16, H=1) [msc-8]
What mass (g) of potassium hydroxide (KOH) is needed to make up 500cm³ of a solution of concentration 4.0mol/dm³? (A_r's: K=39, O=16, H=1) [msc-9]
What mass (g) of hydrogen chloride (HCl) is needed to make up 1000cm³ of a solution of concentration 1mol/dm³? (A_r's: H=1, Cl=35.5) [msc-10]
What mass (g) of hydrogen chloride (HCl) is needed to make up 500cm³ of a solution of concentration 4mol/dm³? (A_r's: H=1, Cl=35.5) [msc-11]
What mass (g) of hydrogen chloride (HCl) is needed to make up 500cm³ of a solution of concentration 0.2mol/dm³? (A_r's: H=1, Cl=35.5) [msc-12]
Given the neutralisation equation:
NaOH_(aq) + HCl_(aq) ==> NaCl_(aq) + H₂O_(l)
25 cm³ of hydrochloric acid are neutralised by 20 cm³ of 0.05M sodium hydroxide. What is the molarity of the acid? [vct-1]
Given the neutralisation equation:
NaOH_(aq) + HCl_(aq) ==> NaCl_(aq) + H₂O_(l)
15 cm³ of hydrochloric acid are neutralised by 25 cm³ of 0.06M sodium hydroxide. What is the molarity of the acid? [vct-2]
Given the neutralisation equation:
NaOH_(aq) + HCl_(aq) ==> NaCl_(aq) + H₂O_(l)
40 cm³ of 0.05M hydrochloric acid are neutralised by 20 cm³ of a sodium hydroxide solution. What is the molarity of the alkali? [vct-3]
Given the neutralisation equation:
NaOH_(aq) + HCl_(aq) ==> NaCl_(aq) + H₂O_(l)
25 cm³ of 0.16M hydrochloric acid are neutralised by 10 cm³ of a sodium hydroxide solution. What is the molarity of the alkali? [vct-4]
Given the neutralisation equation:
2KOH_(aq) + H₂SO_4(aq) ==> K₂SO_4(aq) + 2H₂O_(l)
What is the molarity of a sulphuric acid solution, if 15 cm³ of it are neutralised by 20 cm³ of a 0.3 M potassium hydroxide solution? [vct-5]
Given the neutralisation equation:
2KOH_(aq) + H₂SO_4(aq) ==> K₂SO_4(aq) + 2H₂O_(l)
What is the molarity of a sulphuric acid solution, if 30 cm³ of it are neutralised by 10 cm³ of a 0.6 M potassium hydroxide solution? [vct-6]
Given the neutralisation equation:
2KOH_(aq) + H₂SO_4(aq) ==> K₂SO_4(aq) +2H₂O_(l)
What is the molarity of a potassium hydroxide solution, if 10 cm³ of it are neutralised by 12 cm³ of a 0.5 M sulphuric acid solution? [vct-7]
Given the neutralisation equation:
2KOH_(aq) + H₂SO_4(aq) ==> K₂SO_4(aq) + 2H₂O_(l)
What is the molarity of a potassium hydroxide solution, if 5 cm³ of it are neutralised by 20 cm³ of a 1 M sulphuric acid solution? [vct-8]
Given the neutralisation equation:
3NaOH_(aq) + H₃PO_4(aq) ==> Na₃PO_4(aq) + 3H₂O_(l)
What is the molarity of a phosphoric acid solution, if 15 cm³ of it are neutralised by 22.5 cm³ of a 0.2 M sodium hydroxide solution? [vct-9]
Given the neutralisation equation:
3NaOH_(aq) + H₃PO_4(aq) ==> Na₃PO_4(aq) + 3H₂O_(l)
What is the molarity of a phosphoric acid solution, if 40 cm³ of it are neutralised by 15 cm³ of a 0.4 M sodium hydroxide solution? [vct-10]
Given the neutralisation equation:
3NaOH_(aq) + H₃PO_4(aq) ==> Na₃PO_4(aq) + 3H₂O_(l)
What is the molarity of a sodium hydroxide solution, if 21.6 cm³ of it are neutralised by 18 cm³ of a 0.2 M phosphoric acid solution? [vct-11]
Given the neutralisation equation:
3NaOH_(aq) + H₃PO_4(aq) ==> Na₃PO_4(aq) + 3H₂O_(l)
What is the molarity of a sodium hydroxide solution, if 15 cm³ of it are neutralised by 20 cm³ of a 0.6 M phosphoric acid solution? [vct-12]
Given below are the electrode equations for the electrolysis of aqueous sodium chloride (brine) and the A_r's: H=1 and Cl=35.5:
(-) electrode: 2H⁺_(aq) + 2e^- ==> H_2(g)
(+) electrode: 2Cl^-_(aq) - 2e^- ==> Cl_2(g)
If 2 g of hydrogen was formed at the (-) electrode, what volume (dm³) of chlorine is formed at the (+) electrode? (1 mole of any gas = 24dm³ at room temp./press.) [pec-1]
Given below are the electrode equations for the electrolysis of aqueous sodium chloride (brine) and the A_r's: H=1 and Cl=35.5:
(-) electrode: 2H⁺_(aq) + 2e^- ==> H_2(g)
(+) electrode: 2Cl^-_(aq) - 2e^- ==> Cl_2(g)
If 12 dm³ of hydrogen was formed at the (-) electrode, what mass (g) of chlorine is formed at the (+) electrode? (1 mole of any gas = 24dm³ at room temp./press.) [pec-2]
Given below are the electrode equations for the electrolysis of aqueous sodium chloride (brine) and the A_r's: H=1 and Cl=35.5:
(-) electrode: 2H⁺_(aq) + 2e^- ==> H_2(g)
(+) electrode: 2Cl^-_(aq) - 2e^- ==> Cl_2(g)
If 48 dm³ of chlorine was formed at the (+) electrode, what mass (g) of hydrogen is formed at the (-) electrode? (1 mole of any gas = 24dm³ at room temp./press.) [pec-3]
Given below are the electrode equations for the electrolysis of aqueous sodium chloride (brine) and the A_r's: H=1 and Cl=35.5:
(-) electrode: 2H⁺_(aq) + 2e^- ==> H_2(g)
(+) electrode: 2Cl^-_(aq) - 2e^- ==> Cl_2(g)
If 36 dm³ of chlorine was formed at the (+) electrode, what volume (dm³) of hydrogen is formed at the (-) electrode? (1 mole of any gas = 24dm³ at room temp./press.) [pec-4]
Given below are the electrode equations for the electrolysis of aqueous sodium chloride (brine) and the A_r's: H=1 and Cl=35.5:
(-) electrode: 2H⁺_(aq) + 2e^- ==> H_2(g)
(+) electrode: 2Cl^-_(aq) - 2e^- ==> Cl_2(g)
If 213g of chlorine was formed at the (+) electrode, what volume (dm³) of hydrogen is formed at the (-) electrode? (1 mole of any gas = 24dm³ at room temp./press.) [pec-5]
Given below are the electrode equations for the electrolysis of aqueous sodium chloride (brine) and the A_r's: H=1 and Cl=35.5:
(-) electrode: 2H⁺_(aq) + 2e^- ==> H_2(g)
(+) electrode: 2Cl^-_(aq) - 2e^- ==> Cl_2(g)
If 8 g of hydrogen was formed at the (-) electrode, what mass of chlorine (g) is formed at the (+) electrode? [pec-6]
Given below are the electrode equations for the electrolysis of molten aluminium oxide ore (Al³O₃) and the A_r's: Al=27 and O=16:
(-) electrode: 4Al³⁺_(aq) + 12e^- ==> 4Al_(l)
(+) electrode: 6O^2-_(aq) - 12e^- ==> 3O_2(g)
If 108 g of aluminium is formed at the (-) electrode, what volume (dm³) of oxygen would be formed at the (+) electrode? (1 mole of any gas = 24dm³ at room temp./press.) [pec-7]
Given below are the electrode equations for the electrolysis of molten aluminium oxide ore (Al³O₃) and the A_r's: Al=27 and O=16:
(-) electrode: 4Al³⁺_(aq) + 12e^- ==> 4Al_(l)
(+) electrode: 6O^2-_(aq) - 12e^- ==> 3O_2(g)
If 54 tonne of aluminium is formed at the (-) electrode, what mass (tonne) of oxygen would be formed at the (+) electrode? [pec-8]
Given below are the electrode equations for the electrolysis of molten aluminium oxide ore (Al³O₃) and the A_r's: Al=27 and O=16:
(-) electrode: 4Al³⁺_(aq) + 12e^- ==> 4Al_(l)
(+) electrode: 6O^2-_(aq) - 12e^- ==> 3O_2(g)
If 24 g of oxygen is formed at the (+) electrode, what mass (g) of aluminium would be formed at the (-) electrode? [pec-9]
Given below are the electrode equations for the electrolysis of molten aluminium oxide ore (Al³O₃) and the A_r's: Al=27 and O=16:
(-) electrode: 4Al³⁺_(aq) + 12e^- ==> 4Al_(l)
(+) electrode: 6O^2-_(aq) - 12e^- ==> 3O_2(g)
If 2.7 g of aluminium is formed at the (-) electrode, what volume (dm³) of oxygen would be formed at the (+) electrode? (1 mole of any gas = 24dm³ at room temp./press.) [pec-10]
Given below are the electrode equations for the electrolysis of molten aluminium oxide ore (Al³O₃) and the A_r's: Al=27 and O=16:
(-) electrode: 4Al³⁺_(aq) + 12e^- ==> 4Al_(l)
(+) electrode: 6O^2-_(aq) - 12e^- ==> 3O_2(g)
What mass (g) of aluminium is formed at the (-) electrode, if 72 dm³ of oxygen was formed at the (+) electrode? (1 mole of any gas = 24dm³ at room temp./press.) [pec-11]
Given below are the electrode equations for the electrolysis of molten aluminium oxide ore (Al³O₃) and the A_r's: Al=27 and O=16:
(-) electrode: 4Al³⁺_(aq) + 12e^- ==> 4Al_(l)
(+) electrode: 6O^2-_(aq) - 12e^- ==> 3O_2(g)
If 54 g of aluminium is formed at the (-) electrode, what volume (dm³) of oxygen was formed at the (+) electrode? (1 mole of any gas = 24dm³ at room temp./press.) [pec-12]

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