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When there is an increase in temperature of the system, Le Chatelier’s Principle states that the reaction will shift away from the heat and the energy of the exothermic reaction is favored. On the other hand, a decrease in temperature shifts the reaction toward the heat and the energy of the endothermic reaction is favored.
An easier way to remember this is that if the reaction is endothermic and the temperature is increased, products are formed. If the reaction is exothermic and the temperature is increased, reactants are formed.
Temperature always changes K. If the reaction is endothermic (+ΔH), heating it will favor the formation of products (the forward reaction). If the reaction is exothermic (-ΔH), heating it will favor the formation of reactants (the reverse reaction).
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