Chapter 12, Problem 12.41SP

The oxidation of 2-butanone (CH₃COC₂H₅) by the cerium(IV) ion in aqueous solution to form acetic acid (CH₃CO₂H) occurs according to the following balanced equation:

$\begin{array}{l}{\text{CH}}_3{\text{COC}}_2{\text{H}}_5(aq)+6{\text{Ce}}^{4+}(aq)+3{\text{H}}_2\text{O}(l)\stackrel{}{\to }\\ 2{\text{CH}}_3{\text{CO}}_2\text{H}(aq)+6{\text{Ce}}^{3+}(aq)+6{\text{H}}^{\text{+}}(aq)\end{array}$

1. (a) If acetic acid appears at an average rate of 5.0 × 10⁻⁸ M/s, what is Δ[H⁺]/Δt during the same time interval?
2. (b) What is the average rate of consumption of Ce⁴⁺ during the same time interval?