The position of equilibrium
2 marks · EasyConsider the equilibrium: At equilibrium in a sealed container, there are 2.0 mol of and 4.0 mol of . The forward reaction is exothermic. The temperature is now increased. Calculate the change in the amount of expected at the new equilibrium and explain your answer.
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The amount of CD2 will decrease.
Also accept: CD2 decreases; less CD2; CD2 goes down
Common mistakes: CD2 increases; no change
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Marking points
M1 · 1 mark · States that increasing temperature shifts equilibrium in the endothermic direction (reverse reaction), so less product (CD2) is formed.
A1 · 1 mark · Correctly predicts that the amount of CD2 will decrease/less CD2 at equilibrium.
Worked solution
The forward reaction is exothermic. Increasing the temperature favours the endothermic (reverse) reaction. This means more D2 will form and less CD2 will be present at equilibrium.
Therefore, the amount of CD2 will decrease.