Chapter 20, Problem 20.36E

The rate law for the reaction

${\text{C}}_{\text{6}}{\text{H}}_{\text{5}}\text{OH}+{\text{HNO}}_2\stackrel{\left[{\text{OH}}^{-}\text{catalyst}\right]}{\to }{\text{C}}_{\text{6}}{\text{H}}_{\text{5}}{\text{NO}}_2+{\text{H}}_2\text{O}$

is

$\text{rate}=k\left[{\text{C}}_{\text{6}}{\text{H}}_{\text{5}}\text{OH}\right]\left[{\text{HNO}}_2\right]$

At $35.0°\text{C}$, $k=7.04\times {10}^{-3}{\text{M}}^{-1}{\text{s}}^{-1}$. If $\left[{\text{C}}_{\text{6}}{\text{H}}_{\text{5}}\text{OH}\right]=0.0433\text{M}$ and $\left[{\text{HNO}}_2\right]=6.05\text{M}$, what is the pseudo first-order rate law and what is the value of $k\text{'}$?