Le Chatelier’s Principle: Temperature Changes on Equilibrium Simplified Revision Notes for GCSE AQA Chemistry

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6.2.6 Le Chatelier's Principle: Temperature Changes on Equilibrium

The Effect of Temperature Changes on Equilibrium

According to Le Chatelier's principle, an equilibrium shifts its position to oppose any change in its temperature.

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This means that, when the temperature is increased, the equilibrium will shift towards whichever side of the reaction produces a lower temperature. This reduces the temperature of the reaction and opposes the change.

If the temperature is increased, the equilibrium will shift towards the side of the reaction that absorbs heat (the endothermic side). This helps to reduce the overall temperature.
If the temperature is decreased, the equilibrium will shift towards the side of the reaction that releases heat (the exothermic side) to increase the temperature.

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Example: In the ammonia formation reaction: $N_2+3H_2⇌2NH_3(Δ_fH^∘=−46kJ mol^{-1})$

This reaction is exothermic, meaning the forward reaction releases heat.
If the temperature is increased, the equilibrium will shift to the left, towards the endothermic side (the reactants), to absorb the excess heat, decreasing the concentration of ammonia.
If the temperature is decreased, the equilibrium will shift to the right, towards the exothermic side (the products), to release more heat, increasing the concentration of ammonia.

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