(a(i))[3]
Show, by calculation, which reactant is in excess.
(a(ii))[1]
Describe what you would observe in this reaction.
(b)[2]
The graph shows how the volume of hydrogen gas produced, at room temperature and pressure, varies with time. Calculate the total mass of hydrogen formed.
(c)[2]
The experiment is done again at the same temperature and pressure. The same mass of magnesium is added, but magnesium powder is used rather than small pieces. The reaction rate is higher. Explain why.
(d(i))[1]
When magnesium is heated with nitrogen, the ionic compound magnesium nitride, $\text{Mg}_3\text{N}_2$, is produced. Write the equation for this reaction, including state symbols.
(d(ii))[1]
Deduce the charge on the nitride ion.