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Increasing temperature does not affect activation energy. At a higher temperature, faster moving molecules can collide to overcome the activation energy more frequently. For an exothermic reaction, a higher temperature would favor the reactants, so the forward rate constant would decrease. For an endothermic reaction, a higher temperature would favor the products, so the forward rate constant would increase. This is related to activation energy because a higher temperature favors the direction of the favorable reaction based on which has a higher activation energy (exothermic - higher activation energy for the reverse reaction, endothermic- higher activation energy for the forward reaction).
An increase in temperature doesn't affect the activation energy. In the case of an endothermic reaction, increasing the temperature causes the forward rate constant to increase because it'll be easier to overcome the energy barrier bc there will be more energy (however, the value of the barrier doesn't change). The opposite is true for exothermic – the reverse rate constant increases when temp increases.
If the reaction is endothermic, increasing the temperature lowers the activation energy because it adds energy to the system. For the endothermic reaction this makes it easier for the reactants to form products, this is the opposite for an exothermic reaction.
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