(a)[3]
Calculate how many molecules of nitrogen monoxide are present in 960 dm$^3$ of exhaust gas at room temperature and pressure. One mole of any gas contains $6.02 \times 10^{23}$ molecules.
(b)[1]
Nitrogen and oxygen combine in a car engine to produce nitrogen monoxide. Write the equation for this reaction.
(c)[1]
State one harmful effect caused by oxides of nitrogen in air pollution.
(d)[1]
Describe the way in which oxides of nitrogen produced in a car engine are eliminated by a catalytic converter.
(e(i))[1]
Explain why the diffusion rate of $\text{NO}_2(g)$ is lower than that of $\text{NO}(g)$ when both are under the same conditions.
(e(ii))[1]
The diffusion rate of nitrogen monoxide falls as the temperature falls. Suggest why using ideas from kinetic particle theory.