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The forward reaction is exothermic, so it releases energy. The reverse reaction is endothermic, requiring energy. If temperature is increased, we are inputting heat into the reaction, which will shift towards the left/reactants.
In this reaction heat is on the product side of the reaction. So when you increase the temperature(increase heat) you increase the amount of product. The reaction will shift towards the reactants or shift left.
When looking at an expression you should first determine if it is an endothermic or exothermic reaction and depending on that you can determine how the reaction shifts. When looking at how heat moves around we know that endothermic reactions require heat in the forward direction, and the opposite would be true for an exothermic reaction as well.
In this reaction, heat is on the product side. This indicates that the reverse reaction is endothermic. In this case, an increase in temperature would favor the reactants, caushing a shift to the left.
In an exothermic reaction, the reaction will shift to the left when temperature is increased due to heat already being on the product and needing heat on the reactant side since the reverse reaction is endothermic.
In this scenario, I think of heat as a product. This will make sense as to why it shifts left. On the molecular level, heat is added to the products side of the equation so when heat goes up it increases the number of collisions of products to become reactants.
Because this is an exothermic reaction, an increase in heat will shift to the left because you can basically treat heat as you would treat an increase in a product on the product side. Having an excess of a product on one side will cause the reaction to go towards the reactants side in order to maintain equilibrium.
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