Chapter 12, Problem 12.45SP

The oxidation of Br⁻ by BRO₃⁻, in acidic solution is described by the equation

$5{\text{BR}}^{-}(aq)+{\text{BrO}}_3{}^{-}(aq)+6{\text{H}}^{+}(aq)\stackrel{}{\to }3{\text{Br}}_2(aq)+3{\text{H}}_2\text{O}(l)$

The reaction is first order in Br⁻, first order in BRO₃⁻, and second order in H⁺.

1. (a) Write the rate law.
2. (b) What is the overall reaction order?
3. (c) How does the reaction rate change if the H⁺ concentration is tripled?
4. (d) What is the change in rate if the concentrations of both Br⁻ and BRO₃⁻ are halved?