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