Given the following data, determine the rate law for the reaction
2NO(g) + Cl₂(g) $\rightarrow$ 2NOCl(g) $\begin{array}{cccc}\text { Experiment } & {[\mathrm{NO}](M) } & {[\mathbf{CI_{2}}](M) } & \text { Rate }(M / s) \\1 & 0.0300 & 0.0100 & 3.4 \times 10^{-4} \\2 & 0.0150 & 0.0100 & 8.5 \times 10^{-5} \\3 & 0.0150 & 0.0400 & 3.4 \times 10^{-4}\end{array}$

Question

Given the following data, determine the rate law for the reaction
2NO(g) + Cl₂(g)

\rightarrow

2NOCl(g)

\begin{array}{cccc}\text { Experiment } & {[\mathrm{NO}](M) } & {[\mathbf{CI_{2}}](M) } & \text { Rate }(M / s) \\1 & 0.0300 & 0.0100 & 3.4 \times 10^{-4} \\2 & 0.0150 & 0.0100 & 8.5 \times 10^{-5} \\3 & 0.0150 & 0.0400 & 3.4 \times 10^{-4}\end{array}

Quizplus · Accepted Answer

The rate doubles when [NO] is doubled (experiments 1 and 2), indicating first order with respect to NO. The rate quadruples when [Cl2] is quadrupled (experiments 2 and 3), indicating first order with respect to Cl2. Therefore, the rate law is Rate = k[NO]^2[Cl2].

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