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How will the reaction change if it is exothermic and heat is added (considering the fact that exothermic reactions release heat)? Conversely, how would it change if the reaction was endothermic and cooled (considering that endothermic reactions absorb heat)?
If the reaction is exothermic, then adding heat to the reaction would make the reverse reaction more favorable, and thus more reactants would form. Vice versa for removing heat. If the reaction is endothermic, then adding heat would make the forward reaction more favorable. Vice versa for removing heat.
We can see the exothermic reaction as a reaction with "heat" as a product. Thus if we increase temperature of the system, we are indeed increasing the "concentration" of heat (product), so the reaction goes to the left. It works the same as in an endothermic reaction. We simply see heat as a reactant needed.
You can think of heat like a reactant or product, depending on whether the reaction is endothermic or exothermic, and apply the same rules by Le Chatelier's Principle as you would do with other reactants and products to figure out which way the reaction will shift.
If the reaction is exothermic and heat is added, then the reverse reaction would be favorable, causing more reactants to form. Heat can be seen as a product here, so if heat is added, more reactants will form.
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