Unless $\Delta$H$\degree$_rxn = 0, a change in temperature will affect the value of the equilibrium constant K_c.

Question

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According to Le Chatelier's principle, when a system in equilibrium is subjected to a change in temperature, the system will shift in the direction that minimizes the effect of the change. This means that if the reaction is exothermic (heat is released), an increase in temperature will cause the equilibrium to shift towards the reactants, while a decrease in temperature will cause the equilibrium to shift towards the products. On the other hand, if the reaction is endothermic (heat is absorbed), an increase in temperature will cause the equilibrium to shift towards the products, while a decrease in temperature will cause the equilibrium to shift towards the reactants. Therefore, a change in temperature will affect the position of the equilibrium, and consequently the value of the equilibrium constant K_c.

Unless Δ\DeltaΔ H °\degree° rxn = 0, a Change in Temperature Will Affect the Temperature

Unless $\Delta$ H $\degree$ _rxn = 0, a Change in Temperature Will Affect the Temperature