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When a reaction is exothermic the heat can be considered to be a product, so if the temp increases then the reaction will shift toward the reactants and if the temp decreases then the reaction will shift toward the products. Hope this helps.
A reaction is exothermic when it releases heat. Exothermic reactions have a negative (DELTA H) value. When exothermic reactions are heated they will favor the production of the reactants. Another way to phrase this is that when an exothermic reaction is heated the reaction will move in the reverse direction. Temperature is the only quality that affects the K constant value. In an exothermic reaction, a temperature increase will cause K to decrease.
An exothermic reaction means that the reaction is releasing heat to the surroundings. As a result of the increase in heat, the temperature of the rxn also increases. For an endothermic reaction, the reaction absorbs heat, so the temperature decreases.
Since heat is released in exothermic reactions this means that heat could be considered a product. Increasing the temperature would then be increasing the amount of product, causing a leftward shift to reestablish equilibrium. If temperature is decreased then the forward reaction would occur to reestablish equilibrium.
In an exothermic reaction, since heat is being released as a result of the reactants, increasing the temperature would shift towards those reactants. Vice versa for the products: decreasing temperature would shift towards the products.
If a reaction is exothermic, you can treat heat as a "reactant," where increasing the overall temperature will shift the equilibrium to the left, and decreasing the overall temperature will shift the reaction to the right.
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