The position of equilibrium
2 marks · NormalA reversible reaction is shown below: The forward reaction is exothermic. Explain what will happen to the position of equilibrium if the temperature is increased.
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Also accept: The equilibrium shifts to the left (towards reactants), favouring the endothermic reverse reaction.; Less ammonia (NH3) will be produced at higher temperature because the position of equilibrium moves towards N2 and H2.
Common mistakes: Saying concentrations become equal.; Saying yield increases.
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Marking points
M1 · 1 mark · States that equilibrium shifts to the left (towards reactants)/reverse reaction is favoured.
A1 · 1 mark · Links the shift to the fact that the forward reaction is exothermic/the reverse is endothermic, explaining why temperature increase causes this shift.
Worked solution
Increasing temperature favours the endothermic direction of the reaction. Since the forward reaction is exothermic, the equilibrium will shift to the left, towards the reactants (N2 and H2), to absorb the added heat.