Question

Begin your response to QUESTION I on this page. 1. The following equation represents the decomposition of \( \mathrm{N}_{2} \mathrm{O}_{5} \), for which the rate law is rate \( =k\left[\mathrm{~N}_{2} \mathrm{O}_{5}\right] \cdot \frac{2}{4} \) \[ 2 \mathrm{~N}_{2} \mathrm{O}_{5}(g) \rightarrow 4 \mathrm{NO}_{2}(g)+\mathrm{O}_{2}(g) \] A sample of pure \( \mathrm{N}_{2} \mathrm{O}_{5}(g) \) is placed in an evacuated container and allowed to decompose at a constant temperature of 300 K . The concentration of \( \mathrm{N}_{2} \mathrm{O}_{5}(g) \) in the container is measured over a period of time, and the measurements are recorded in the following table. \begin{tabular}{|c|c|} \hline Time \( (\mathrm{hr}) \) & {\( \left[\mathrm{N}_{2} \mathrm{O}_{5}\right](M) \)} \\ \hline 0 & 0.160 \\ \hline 1.67 & 0.0800 \\ \hline 3.33 & 0.0400 \\ \hline 5.00 & 0.0200 \\ \hline \end{tabular} (a) Determine the value of the rate constant, \( k \), for the reaction. Include units in your answer.

          Begin your response to QUESTION I on this page.
1. The following equation represents the decomposition of \( \mathrm{N}_{2} \mathrm{O}_{5} \), for which the rate law is rate \( =k\left[\mathrm{~N}_{2} \mathrm{O}_{5}\right] \cdot \frac{2}{4} \)
\[
2 \mathrm{~N}_{2} \mathrm{O}_{5}(g) \rightarrow 4 \mathrm{NO}_{2}(g)+\mathrm{O}_{2}(g)
\]

A sample of pure \( \mathrm{N}_{2} \mathrm{O}_{5}(g) \) is placed in an evacuated container and allowed to decompose at a constant temperature of 300 K . The concentration of \( \mathrm{N}_{2} \mathrm{O}_{5}(g) \) in the container is measured over a period of time, and the measurements are recorded in the following table.
\begin{tabular}{|c|c|}
\hline Time \( (\mathrm{hr}) \) & {\( \left[\mathrm{N}_{2} \mathrm{O}_{5}\right](M) \)} \\
\hline 0 & 0.160 \\
\hline 1.67 & 0.0800 \\
\hline 3.33 & 0.0400 \\
\hline 5.00 & 0.0200 \\
\hline
\end{tabular}
(a) Determine the value of the rate constant, \( k \), for the reaction. Include units in your answer.

Begin your response to QUESTION I on this page.
1. The following equation represents the decomposition of N2O5, for which the rate law is rate =k[ N2O5] ·(2)/(4)

2 N2O5(g) → 4 NO2(g)+O2(g)

A sample of pure N2O5(g) is placed in an evacuated container and allowed to decompose at a constant temperature of 300 K . The concentration of N2O5(g) in the container is measured over a period of time, and the measurements are recorded in the following table.

Time (hr) [N2O5](M)

0 0.160

1.67 0.0800

3.33 0.0400

5.00 0.0200

(a) Determine the value of the rate constant, k, for the reaction. Include units in your answer.

Added by Gregg M.

Question

Please give Ace some feedback