(a(i))[2]
Calculate the volume of hydrogen produced at room temperature and pressure when excess sulfuric acid reacts with a $0.65\,\text{g}$ sample of zinc.
(a(ii))[1]
Explain why a different volume of hydrogen is produced when $0.65\,\text{g}$ of iron is reacted with excess sulfuric acid.
(b)[4]
Describe what you would observe as aqueous sodium hydroxide is added to the reaction mixture, and explain what reactions are occurring.
(c(i))[1]
Explain how you know that oxidation is taking place in the reaction.
(c(ii))[2]
Describe the chemical test for sulfur dioxide and state what you observe.