Question

digits. \begin{tabular}{|c|c|c|} \hline\( \left[\mathrm{N}_{2}\right] \) & {\( \left[\mathrm{H}_{2}\right] \)} & initial rate of reaction \\ \hline 0.684 M & 2.06 M & \( 8.00 \mathrm{M} / \mathrm{s} \) \\ \hline 0.684 M & 0.731 M & \( \square \mathrm{M} / \mathrm{s} \) \\ \hline 0.178 M & 7.93 M & \( \square \mathrm{M} / \mathrm{s} \) \\ \hline \end{tabular}

          digits.
\begin{tabular}{|c|c|c|}
\hline\( \left[\mathrm{N}_{2}\right] \) & {\( \left[\mathrm{H}_{2}\right] \)} & initial rate of reaction \\
\hline 0.684 M & 2.06 M & \( 8.00 \mathrm{M} / \mathrm{s} \) \\
\hline 0.684 M & 0.731 M & \( \square \mathrm{M} / \mathrm{s} \) \\
\hline 0.178 M & 7.93 M & \( \square \mathrm{M} / \mathrm{s} \) \\
\hline
\end{tabular}

digits.

[N2] [H2] initial rate of reaction

0.684 M 2.06 M 8.00 M / s

0.684 M 0.731 M □M / s

0.178 M 7.93 M □M / s

Added by Darnell C.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Adedamola Opalade

Step 1

The reaction is first order in \( \text{N}_2 \) and second order in \( \text{H}_2 \). Therefore, the rate law is: \[ \text{Rate} = k [\text{N}_2]^1 [\text{H}_2]^2 \] Show more…

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digits. \begin{tabular}{|c|c|c|} \hline\( \left[\mathrm{N}_{2}\right] \) & {\( \left[\mathrm{H}_{2}\right] \)} & initial rate of reaction \\ \hline 0.684 M & 2.06 M & \( 8.00 \mathrm{M} / \mathrm{s} \) \\ \hline 0.684 M & 0.731 M & \( \square \mathrm{M} / \mathrm{s} \) \\ \hline 0.178 M & 7.93 M & \( \square \mathrm{M} / \mathrm{s} \) \\ \hline \end{tabular}