Ammonia is manufactured in the Haber process by the reversible reaction between nitrogen and hydrogen. The graph shows the equilibrium percentage of ammonia at different temperatures and pressures.

1. aWrite the equation for this reaction including state symbols. [3]
2. bState the conditions necessary for the Haber process: catalyst, temperature and pressure. [3]
3. cUse the graph to deduce the relationship between the equilibrium percentage of ammonia and increasing temperature, and increasing pressure. [2]
4. dUse your answer above to state whether the forward reaction is endothermic or exothermic and explain why. [1]
5. eExplain why the continuous removal of ammonia from the equilibrium mixture increases the yield. [1]

You'll mark your own answer against the marking guide when you hand it in.