(a)[2]
Draw a ‘dot-and-cross’ diagram that represents the $\text{ClNO}_2$ molecule.
(b(i))[1]
Write the rate equation that applies to this reaction.
(b(ii))[1]
Deduce the units of the rate constant, $k$, when both gas concentrations are given in $\text{mol dm}^{-3}$ and the rate is given in $\text{mol dm}^{-3}\ \text{s}^{-1}$.
(b(iii))[1]
State and explain whether or not the reaction could take place in a single step.
(c(i))[2]
Draw a graph on the grid to show how the concentration of $\text{ClNO}_2$ changes over the first $0.20\ \text{s}$.
(c(ii))[1]
Deduce the concentration of the $\text{NO}_2$ product at $0.20\ \text{s}$.
(c(iii))[1]
After $20\ \text{s}$ the concentration of $\text{ClNO}_2$ remains constant. Explain this observation.