Write an equation that shows the reaction taking place in stage 1.
Draw a ‘dot-and-cross’ diagram to show how the outer electrons are arranged in a molecule of ammonia.
In the boxes, give the oxidation numbers of nitrogen in the nitrogen-containing species for the reaction in stage 3, $\text{3NO}_2 + \text{H}_2\text{O} \rightarrow 2\text{HNO}_3 + \text{NO}$.
Explain why the reaction in stage 3 is called a disproportionation reaction. Include reference to electron transfer in your answer.
The release of nitrogen monoxide into the atmosphere leads to atmospheric pollution. State and explain the effect of nitrogen monoxide gas when it comes into contact with moist air.
The nitric acid formed in stage 3 can then be reacted with ammonia to make ammonium nitrate. Stage 3: $3\text{NO}_2 + \text{H}_2\text{O} \rightarrow 2\text{HNO}_3 + \text{NO}$. $\text{NH}_3 + \text{HNO}_3 \rightarrow \text{NH}_4\text{NO}_3$. Calculate the volume of nitrogen dioxide, measured at room temperature and pressure, needed to make $40$ tonnes of ammonium nitrate. [$1$ tonne $= 1000\,\text{kg}$]. Show your working.
State one use of ammonium nitrate.