Question detail
In a reversible reaction, the forward reaction is exothermic. If the temperature is increased, predict the effect on the position of equilibrium and justify your answer using Le Chatelier's Principle.
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At a glance
Question
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Topic
Reversible reactions and dynamic equilibrium
Question
In a reversible reaction, the forward reaction is exothermic. If the temperature is increased, predict the effect on the position of equilibrium and justify your answer using Le Chatelier's Principle.
Answer
Increasingthe temperature will shift the equilibrium position to the left, favoringthe endothermicdirection, which produces more reactants.
Explanation
This answer reflects the application of Le chatelier's Principle, indicatingthat increasingtemperature causes the system to shift in the direction that absorbs heat, thus favoringthe endothermicreaction. This answer is strongest when it stays anchored to The effect of temperature changes on equilibrium (HT only) and directly addresses (HT only) Predict that decreasingtemperature favours the exothermicdirection of a reversible reaction.
Common mistake
Misunderstanding Temperature Effects
Students often think that decreasing temperature always increases the rate of reaction instead of favouring the exothermic direction of a reversible reaction.
Remember that decreasing temperature favours the exothermic direction, which can lead to increased product yield, but it does not necessarily mean the reaction rate will increase.
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