For the following reaction, state order of reaction with respect to each reactant and the overall order of reaction.${\mathrm{CH}}_3{\mathrm{COCH}}_3 + {\mathrm{I}}_2 \stackrel{{\mathrm{H}}^{+}}{\to } {\mathrm{CH}}_3{\mathrm{COCH}}_2\mathrm{I} + \mathrm{HI}$ where rate is proportional to the concentration of ${\mathrm{CH}}_3{\mathrm{COCH}}_3$ and to the concentration of${\mathrm{H}}^{+}$ ions, but the concentration of ${\mathrm{I}}_2$ has no effect on the rate.

State the units of $\mathrm{k}$ corresponding to each of the following rate equation:

Rate $= \mathrm{k}{\left[\mathrm{NO}\right]}^2$

State the units of $\mathrm{k}$ corresponding to each of the following rate equation:

Rate $= \mathrm{k}{\left[{\mathrm{NH}}_3\right]}^0$

State the units of $\mathrm{k}$ corresponding to each of the following rate equation:

Rate $= \mathrm{k}[{{\mathrm{BrO}}_3}^{–} ][{\mathrm{Br}}^{–} ]{\left[{\mathrm{H}}^{+}\right]}^2$

State the units of $\mathrm{k}$ corresponding to each of the following rate equation:

Rate $= \mathrm{k}\left[\mathrm{cyclopropane}\right]$

Draw sketch graphs of reaction rate against concentration of the reactant in bold for each of the following reaction:

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

Draw sketch graphs of reaction rate against concentration of the reactant in bold for each of the following reaction:

$2\mathbf{HI}\left(\mathrm{g}\right) \stackrel{\mathrm{gold}}{\to } {\mathrm{H}}_2\left(\mathrm{g}\right) + {\mathrm{I}}_2\left(\mathrm{g}\right)$ 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 sketch graphs of reaction rate against concentration of the reactant in bold for each of the following reaction:

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

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$= \mathrm{k}{\left[\mathrm{NO}\right]}^2$