The data below were determined for the reaction shown below.S₂O₈^2- + 3I ^- (aq) $\rarr$ 2SO₄^2- + I₃^-

$\begin{array}{lccc}\text { Expt. \# } & \left[\mathrm{S}_{2-} \mathrm{O}_{8}{ }^{2}\right] & {[I-]} & \text { Initial Rate } \\\hline 1 & 0.038 & 0.060 & 1.4 \times 10^{-5} \mathrm{M} / \mathrm{s} \\2 & 0.076 & 0.060 & 2.8 \times 10^{-5} \mathrm{M} / \mathrm{s} \\3 & 0.076 & 0.030 & 1.4 \times 10^{-5} \mathrm{M} / \mathrm{s}\end{array}$ The rate law for this reaction must be:

Question

The data below were determined for the reaction shown below.S₂O₈^2- + 3I ^- (aq)

\rarr

2SO₄^2- + I₃^-

\begin{array}{lccc}\text { Expt. \# } & \left[\mathrm{S}_{2-} \mathrm{O}_{8}{ }^{2}\right] & {[I-]} & \text { Initial Rate } \\\hline 1 & 0.038 & 0.060 & 1.4 \times 10^{-5} \mathrm{M} / \mathrm{s} \\2 & 0.076 & 0.060 & 2.8 \times 10^{-5} \mathrm{M} / \mathrm{s} \\3 & 0.076 & 0.030 & 1.4 \times 10^{-5} \mathrm{M} / \mathrm{s}\end{array}

The rate law for this reaction must be:

Quizplus · Accepted Answer

The rate law for this reaction has a stoichiometric coefficient of 1 for both reactants, which indicates a simple first-order reaction. Therefore, the rate law must have the form rate = k[A][B], where A is the concentration of S₂O₈^2- and B is the concentration of I ^-. Option E is the only one that matches this form.

The Data Below Were Determined for the Reaction Shown Below →\rarr→

The Data Below Were Determined for the Reaction Shown Below $\rarr$