(a(i))[2]
State the temperature and pressure applied in the Haber process.
(a(ii))[1]
Name the catalyst employed in the Haber process.
(b(i))[2]
Complete the balancing of this equation: $4\text{NH}_3 + \ldots\text{O}_2 \rightleftharpoons \ldots\text{NO} + \ldots\text{H}_2\text{O}$.
(b(ii))[1]
Suggest a reason, apart from cost, why a temperature above $900\,^{\circ}\text{C}$ is not chosen.
(b(iii))[1]
Suggest a reason why a temperature below $900\,^{\circ}\text{C}$ is not chosen.
(c)[2]
Write a chemical equation for the reaction described.
(d)[6]
Describe how you would prepare a pure dry sample of copper(II) nitrate crystals in the laboratory using dilute nitric acid and solid copper(II) carbonate. In your response, give a sequence of key steps. You should include a chemical equation for the reaction.