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When you increase the temperature of an exothermic reaction, it is known to shift left. I understand this fact, but have trouble conceptualizing it and understanding precisely WHY. Why wouldn’t an exothermic reaction with added heat shift right since its inclined to release heat?
an exothermic reaction releases heat which means heat is a product in a chemical reaction. when you increase the temperature, think of it like you are increasing the amount of product. when more product is added, the equilibrium shifts towards the left.
It might help if you view heat as another reactant (for an endothermic reaction) or as another product (for an exothermic reaction). If you add more of a reactant, according to Le Chatelier's, the effect of the change will need to be minimized so the reaction will proceed to the right. So in an endothermic reaction, you have heat on the left side of your equation so adding more heat to the system will make the reaction go away from the left side (favoring products). In an exothermic reaction, you have heat on the right side of your equation so adding more heat to the system will make it proceed away from the right side (favoring reactants).
Exothermic reactions give off heat while forming product, and reactant formation will be favored. For exothermic reactions, you can picture heat as being a product and apply Le Chatelier's principle of what happens when you add product to a system. Therefore, increasing the temperature will shift the equilibrium to the left towards reactants.
Thank you for asking and thank you for the explanations!
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