1.1. During the following reaction, A and B react together to produce C. 

A + 2B → C

The production of C over time is shown below.

i) Sketch a line on the graph to show what happens to A and B during the progress of the reaction. 

[1]

ii) On the graph, write the letter E at the point at which an equilibrium is first established.

[1]

1.2. In the reaction in part (a), lumps of A were used. Use collision theory to explain what would happen to the rate of the reaction if powdered A was used instead of lumps. 

1.3. Hydrogen peroxide decomposes more rapidly in the presence of aqueous hydrogen bromide. The decomposition proceeds as shown by the following equations.

H₂O₂ + HBr  →  HBrO + H₂O

HBrO + H₂O₂ →  H₂O + O₂ + HBr

Give two reasons, other than an increase in the reaction rate, why these equations suggest that hydrogen bromide is behaving as a catalyst.

1.4. In the Haber Process, nitrogen and hydrogen are reacted together in a sealed container to form ammonia, NH₃. Increasing the pressure and adding a catalyst both speed up the rate of this reaction.

i) Write a balanced symbol equation to show this reaction.

[1]

ii) Explain why, using collision theory, increasing the pressure speeds up the rate of the reaction.

[2]

iii) Use a labelled Maxwell-Boltzmann curve to explain how the addition of a catalyst increases the rate of reaction.

[3]