Chapter 20, Problem 20.2E

The oxidation-reduction reaction between iron metal and aqueous permanganate ions in acidic solution is

$\begin{array}{l}16{\text{H}}^{+}\left(\text{aq}\right)+5\text{Fe}\left(\text{s}\right)+2{\text{MnO}}_4{}^{-}\left(\text{aq}\right)\to \\ 2{\text{Mn}}^{2+}\left(\text{aq}\right)+5{\text{Fe}}^{2+}+8{\text{H}}_2\text{O}\left(l\right)\end{array}$ At some temperature, the reaction proceeds at such a rate that $1.00$ millimole of ${\text{H}}^{+}$ is consumed in $2$ minutes $33.8$ seconds. What is the (invariant) rate of this reaction in units of moles per second?