(1) Whenever a chemical reaction take place there is also an accompanying co-existcollideconditionsconstantdecreaseddynamicdynamic equilibriumendothermicendothermic reactionenergy changeequilibriumexothermicexothermic reactionheatedincreasedpositionproductsreactantsreaction conditionsrearrangedreversible. If the reaction gives out heat to the surroundings it is called an co-existcollideconditionsconstantdecreaseddynamicdynamic equilibriumendothermicendothermic reactionenergy changeequilibriumexothermicexothermic reactionheatedincreasedpositionproductsreactantsreaction conditionsrearrangedreversible and the temperature is co-existcollideconditionsconstantdecreaseddynamicdynamic equilibriumendothermicendothermic reactionenergy changeequilibriumexothermicexothermic reactionheatedincreasedpositionproductsreactantsreaction conditionsrearrangedreversible.

(2) If heat energy is absorbed by the reactants its known as an co-existcollideconditionsconstantdecreaseddynamicdynamic equilibriumendothermicendothermic reactionenergy changeequilibriumexothermicexothermic reactionheatedincreasedpositionproductsreactantsreaction conditionsrearrangedreversible. and either the temperature is co-existcollideconditionsconstantdecreaseddynamicdynamic equilibriumendothermicendothermic reactionenergy changeequilibriumexothermicexothermic reactionheatedincreasedpositionproductsreactantsreaction conditionsrearrangedreversible by absorbing heat from the surroundings, or the reactants must be co-existcollideconditionsconstantdecreaseddynamicdynamic equilibriumendothermicendothermic reactionenergy changeequilibriumexothermicexothermic reactionheatedincreasedpositionproductsreactantsreaction conditionsrearrangedreversible to effect the chemical change.

(3) When reactant molecules co-existcollideconditionsconstantdecreaseddynamicdynamic equilibriumendothermicendothermic reactionenergy changeequilibriumexothermicexothermic reactionheatedincreasedpositionproductsreactantsreaction conditionsrearrangedreversible to react, bonds must be broken and new bonds formed to give the products as the atoms are co-existcollideconditionsconstantdecreaseddynamicdynamic equilibriumendothermicendothermic reactionenergy changeequilibriumexothermicexothermic reactionheatedincreasedpositionproductsreactantsreaction conditionsrearrangedreversible. Bond breaking is an co-existcollideconditionsconstantdecreaseddynamicdynamic equilibriumendothermicendothermic reactionenergy changeequilibriumexothermicexothermic reactionheatedincreasedpositionproductsreactantsreaction conditionsrearrangedreversible process and bond making is an co-existcollideconditionsconstantdecreaseddynamicdynamic equilibriumendothermicendothermic reactionenergy changeequilibriumexothermicexothermic reactionheatedincreasedpositionproductsreactantsreaction conditionsrearrangedreversible process.

(4) You normally think of a chemical reaction in terms of co-existcollideconditionsconstantdecreaseddynamicdynamic equilibriumendothermicendothermic reactionenergy changeequilibriumexothermicexothermic reactionheatedincreasedpositionproductsreactantsreaction conditionsrearrangedreversible ====> co-existcollideconditionsconstantdecreaseddynamicdynamic equilibriumendothermicendothermic reactionenergy changeequilibriumexothermicexothermic reactionheatedincreasedpositionproductsreactantsreaction conditionsrearrangedreversible, but sometimes the reaction is co-existcollideconditionsconstantdecreaseddynamicdynamic equilibriumendothermicendothermic reactionenergy changeequilibriumexothermicexothermic reactionheatedincreasedpositionproductsreactantsreaction conditionsrearrangedreversible and the products can change back into the reactants if the co-existcollideconditionsconstantdecreaseddynamicdynamic equilibriumendothermicendothermic reactionenergy changeequilibriumexothermicexothermic reactionheatedincreasedpositionproductsreactantsreaction conditionsrearrangedreversible are changed.

(5) In other situations a reaction does not go to completion and the reactants and products all co-existcollideconditionsconstantdecreaseddynamicdynamic equilibriumendothermicendothermic reactionenergy changeequilibriumexothermicexothermic reactionheatedincreasedpositionproductsreactantsreaction conditionsrearrangedreversible with each other. However, the reaction hasn't stopped and reactants change to co-existcollideconditionsconstantdecreaseddynamicdynamic equilibriumendothermicendothermic reactionenergy changeequilibriumexothermicexothermic reactionheatedincreasedpositionproductsreactantsreaction conditionsrearrangedreversible and products change into the original co-existcollideconditionsconstantdecreaseddynamicdynamic equilibriumendothermicendothermic reactionenergy changeequilibriumexothermicexothermic reactionheatedincreasedpositionproductsreactantsreaction conditionsrearrangedreversible. Eventually the concentrations of reactants and products remain co-existcollideconditionsconstantdecreaseddynamicdynamic equilibriumendothermicendothermic reactionenergy changeequilibriumexothermicexothermic reactionheatedincreasedpositionproductsreactantsreaction conditionsrearrangedreversible, but the two reactions continue and maintain what is called a co-existcollideconditionsconstantdecreaseddynamicdynamic equilibriumendothermicendothermic reactionenergy changeequilibriumexothermicexothermic reactionheatedincreasedpositionproductsreactantsreaction conditionsrearrangedreversible co-existcollideconditionsconstantdecreaseddynamicdynamic equilibriumendothermicendothermic reactionenergy changeequilibriumexothermicexothermic reactionheatedincreasedpositionproductsreactantsreaction conditionsrearrangedreversible (a state of concentration balance).

(6) The position of an co-existcollideconditionsconstantdecreaseddynamicdynamic equilibriumendothermicendothermic reactionenergy changeequilibriumexothermicexothermic reactionheatedincreasedpositionproductsreactantsreaction conditionsrearrangedreversible (reactants <==> products) can be changed by changing the co-existcollideconditionsconstantdecreaseddynamicdynamic equilibriumendothermicendothermic reactionenergy changeequilibriumexothermicexothermic reactionheatedincreasedpositionproductsreactantsreaction conditionsrearrangedreversible under which the reaction takes place.

(7) If a reaction is endothermic, the reaction is favoured if the temperature of the system is co-existcollideconditionsconstantdecreaseddynamicdynamic equilibriumendothermicendothermic reactionenergy changeequilibriumexothermicexothermic reactionheatedincreasedpositionproductsreactantsreaction conditionsrearrangedreversible.

(8) If the reaction is exothermic, the reaction is favoured if the temperature of the reaction is co-existcollideconditionsconstantdecreaseddynamicdynamic equilibriumendothermicendothermic reactionenergy changeequilibriumexothermicexothermic reactionheatedincreasedpositionproductsreactantsreaction conditionsrearrangedreversible.

(9) In a reaction, the side of the equilibrium with the least number of gas molecules in the equation is favoured by co-existcollideconditionsconstantdecreaseddynamicdynamic equilibriumendothermicendothermic reactionenergy changeequilibriumexothermicexothermic reactionheatedincreasedpositionproductsreactantsreaction conditionsrearrangedreversible pressure.

(10) Changing concentrations can also change the co-existcollideconditionsconstantdecreaseddynamicdynamic equilibriumendothermicendothermic reactionenergy changeequilibriumexothermicexothermic reactionheatedincreasedpositionproductsreactantsreaction conditionsrearrangedreversible of an equilibrium. If the concentration of reactants is increased then more co-existcollideconditionsconstantdecreaseddynamicdynamic equilibriumendothermicendothermic reactionenergy changeequilibriumexothermicexothermic reactionheatedincreasedpositionproductsreactantsreaction conditionsrearrangedreversible will be formed to reform the co-existcollideconditionsconstantdecreaseddynamicdynamic equilibriumendothermicendothermic reactionenergy changeequilibriumexothermicexothermic reactionheatedincreasedpositionproductsreactantsreaction conditionsrearrangedreversible.