Lawrie Ryan and Roger Norris Solutions for Chapter: Reaction Kinetics, Exercise 7: Question

Draw a sketch graph to show how the concentration of the bold reactant changes with time.

$\mathbf{NO}\mathbf{\left(}\mathrm{g}\right) + \mathrm{CO}\left(\mathrm{g}\right) + {\mathrm{O}}_2\left(\mathrm{g}\right) \to {\mathrm{NO}}_2\left(\mathrm{g}\right) + {\mathrm{CO}}_2\left(\mathrm{g}\right)$ for which the rate equation is: rate$= \mathrm{k}{\left[\mathrm{NO}\right]}^2$

Draw a sketch graph to show how the concentration of the bold reactant changes with time.

$2\mathbf{HI}\left(\mathrm{g}\right) \stackrel{\mathrm{gold}}{\to } {\mathrm{H}}_2\left(\mathrm{g}\right) + {\mathrm{I}}_2\left(\mathrm{g}\right)$ for which the rate equation is: $\mathrm{rate} = \mathrm{k}$

Note: the catalyst influences the order here – the order is not the same as for the uncatalysed reaction

Draw a sketch graph to show how the concentration of the bold reactant changes with time.

${\mathbf{\left(}{\mathbf{CH}}_{\mathbf{3}}\mathbf{\right)}}_{\mathbf{3}}\mathbf{CCl} + {\mathrm{OH}}^{–} \to {\left({\mathrm{CH}}_3\right)}_3\mathrm{COH} + {\mathrm{Cl}}^{–}$ for which the rate equation is: $\mathrm{k}\left[{\left({\mathrm{CH}}_3\right)}_3\mathrm{CCl}\right]$