Given the following data, determine the rate law for the reaction
NH₄⁺(aq) + NO₂^-(aq) $\rightarrow$ N₂(g) + 2H₂O(l) $\begin{array}{cccc}\text { Experiment } & {\left[\mathrm{NH}_{4}^{+}\right](\boldsymbol{M}) } & {\left[\mathrm{NO}_{2}{ }^{-}\right](\boldsymbol{M}) } & \text { Rate }(\boldsymbol{M} / \mathbf{s}) \\1 & 0.2500 & 0.2500 & 1.25 \times 10^{-3} \\2 & 0.5000 & 0.2500 & 2.50 \times 10^{-3} \\3 & 0.2500 & 0.1250 & 6.25 \times 10^{-4}\end{array}$

Question

Given the following data, determine the rate law for the reaction
NH₄⁺(aq) + NO₂^-(aq)

\rightarrow

N₂(g) + 2H₂O(l)

\begin{array}{cccc}\text { Experiment } & {\left[\mathrm{NH}_{4}^{+}\right](\boldsymbol{M}) } & {\left[\mathrm{NO}_{2}{ }^{-}\right](\boldsymbol{M}) } & \text { Rate }(\boldsymbol{M} / \mathbf{s}) \\1 & 0.2500 & 0.2500 & 1.25 \times 10^{-3} \\2 & 0.5000 & 0.2500 & 2.50 \times 10^{-3} \\3 & 0.2500 & 0.1250 & 6.25 \times 10^{-4}\end{array}

Quizplus · Accepted Answer

The rate law is first order in NH4+ and first order in NO2-. This is because the rate of the reaction is directly proportional to the concentration of each reactant.

Given the Following Data, Determine the Rate Law for the Reaction