d) The back reaction in Equation 1, in which NO2 reacts to give NO and O2, was investigated in t

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This question is really just asking what happens when we double the concentration of NO2. If the

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d) The back reaction in Equation 1, in which \( \mathrm{NO}_{2} \) reacts to give NO and \( \mathrm{O}_{2} \), was investigated in two separate kinetic studies at different temperatures. Below are data from these studies, both of which begin with pure \( \mathrm{NO}_{2} \) (initial concentration of NO and \( \mathrm{O}_{2} \) is zero). Determine the rate law for the back reaction, and calculate the rate constants \( k \) at \( 300^{\circ} \mathrm{C} \) and \( 383^{\circ} \mathrm{C} \). Table 2. Concentration of \( \mathrm{NO}_{2} \) as a function of time at \( 300^{\circ} \mathrm{C} \). \begin{tabular}{ll} Time (s) & {\( \left[\mathrm{NO}_{2}\right](\mathrm{M}) \)} \\ 0 & 0.01000 \\ 50 & 0.00787 \\ 100 & 0.00649 \\ 200 & 0.00481 \\ 300 & 0.00380 \end{tabular} Table 3. Concentration of \( \mathrm{NO}_{2} \) as a function of time at \( 383^{\circ} \mathrm{C} \). \begin{tabular}{ll} Time \( (\mathrm{s}) \) & {\( \left[\mathrm{NO}_{2}\right](\mathrm{M}) \)} \\ 0 & 0.100 \\ 5 & 0.017 \\ 10 & 0.0090 \\ 15 & 0.0062 \\ 20 & 0.0047 \end{tabular}

          d) The back reaction in Equation 1, in which \( \mathrm{NO}_{2} \) reacts to give NO and \( \mathrm{O}_{2} \), was investigated in two separate kinetic studies at different temperatures. Below are data from these studies, both of which begin with pure \( \mathrm{NO}_{2} \) (initial concentration of NO and \( \mathrm{O}_{2} \) is zero). Determine the rate law for the back reaction, and calculate the rate constants \( k \) at \( 300^{\circ} \mathrm{C} \) and \( 383^{\circ} \mathrm{C} \).

Table 2. Concentration of \( \mathrm{NO}_{2} \) as a function of time at \( 300^{\circ} \mathrm{C} \).
\begin{tabular}{ll} 
Time (s) & {\( \left[\mathrm{NO}_{2}\right](\mathrm{M}) \)} \\
0 & 0.01000 \\
50 & 0.00787 \\
100 & 0.00649 \\
200 & 0.00481 \\
300 & 0.00380
\end{tabular}

Table 3. Concentration of \( \mathrm{NO}_{2} \) as a function of time at \( 383^{\circ} \mathrm{C} \).
\begin{tabular}{ll} 
Time \( (\mathrm{s}) \) & {\( \left[\mathrm{NO}_{2}\right](\mathrm{M}) \)} \\
0 & 0.100 \\
5 & 0.017 \\
10 & 0.0090 \\
15 & 0.0062 \\
20 & 0.0047
\end{tabular}

d) The back reaction in Equation 1, in which NO2 reacts to give NO and O2, was investigated in two separate kinetic studies at different temperatures. Below are data from these studies, both of which begin with pure NO2 (initial concentration of NO and O2 is zero). Determine the rate law for the back reaction, and calculate the rate constants k at 300^∘C and 383^∘C.

Table 2. Concentration of NO2 as a function of time at 300^∘C.

Time (s) [NO2](M)

0 0.01000

50 0.00787

100 0.00649

200 0.00481

300 0.00380

Table 3. Concentration of NO2 as a function of time at 383^∘C.

Time (s) [NO2](M)

0 0.100

5 0.017

10 0.0090

15 0.0062

20 0.0047

Added by Margaret P.

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