(a)[2]
Calculate the mass of zinc in $30.0$ tonnes of $\text{ZnS}$.
(b(i))[2]
When $\text{ZnS}$ is heated in air, zinc oxide and sulfur dioxide are produced. Construct the equation for this reaction.
(b(ii))[1]
Suggest one environmental problem involved with heating $\text{ZnS}$ in air.
(c)[1]
Zinc oxide is reacted with dilute sulfuric acid to form aqueous zinc sulfate. Construct the equation for this reaction.
(d)[2]
Pure zinc is produced by electrolysis of aqueous zinc sulfate. Zinc is formed at the negative electrode, while hydroxide ions react at the positive electrode. Construct the equations for the reactions at both electrodes.
(e)[2]
Zinc is used to galvanise iron to prevent the iron from rusting. Explain how galvanising prevents iron from rusting.