Nitrosyl bromide decomposes by the reaction 2 NOBr(g) → 2 NO(g) + Br₂(g). Show that the following data are consistent with a second-order reaction and determine the second-order rate constant for the reaction. Students may do this by plotting the data three different ways. For each plot, time goes on the x-axis. zero-order reaction is linear when [NOBr] on the y-axis. first-order reaction is linear when In[NOBr] is on the y-axis. second-order reaction is linear when 1/[NOBr] is on the y-axis. t 0 5 10 15 50 85 [NOBr] 0.0653 0.0514 0.0424 0.0361 0.0177 0.0117 M What is the rate law for the reaction? (Rate equations take the general form 'rate = k. [A]. [B]'.) What is the value of the rate constant at the temperature of the experiment? What are the units for the rate law? OM-2.5-1 OM-3.5-1 OM-².5-2 O M-1. s-1 chemPad XX→ ← Help Greek

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**Topic: Reaction Kinetics and Rate Laws**

*Overview:*

Nitrosyl bromide decomposes by the reaction \( 2 \text{NOBr}(g) \rightarrow 2 \text{NO}(g) + \text{Br}_2(g) \). The objective is to show that the following data are consistent with a second-order reaction and determine the second-order rate constant for the reaction.

*Data Presentation:*

- The reaction data can be analyzed by plotting the data in three different ways.
- For each plot, time \( t \) goes on the x-axis.
- A zero-order reaction is linear when \([\text{NOBr}]\) is on the y-axis.
- A first-order reaction is linear when \(\ln([\text{NOBr}])\) is on the y-axis.
- A second-order reaction is linear when \(1/[\text{NOBr}]\) is on the y-axis.

*Given Data:*

\[
\begin{array}{c|cccccc}
t \text{ (s)} & 0 & 5 & 10 & 15 & 50 & 85 \\
\hline
[\text{NOBr}] \text{ (M)} & 0.0653 & 0.0514 & 0.0424 & 0.0361 & 0.0177 & 0.0117 \\
\end{array}
\]

*Questions:*

1. What is the rate law for the reaction? (Rate equations take the general form 'rate = k \cdot [A] \cdot [B]^n'.)
   
   - The reaction is determined to be second order, indicated by a linear plot of \(1/[\text{NOBr}]\) vs. time.

2. What is the value of the rate constant at the temperature of the experiment?

   - The rate constant \( k \) is given as 49.0.

3. What are the units for the rate law?

   - Options provided:
     - \( \text{M}^{-2} \cdot \text{s}^{-1} \)
     - \( \text{M}^{-3} \cdot \text{s}^{-1} \)
     - \( \text{M}^{-2} \cdot \text{s}^{-2} \)
     - \( \text{
Transcribed Image Text:**Topic: Reaction Kinetics and Rate Laws** *Overview:* Nitrosyl bromide decomposes by the reaction \( 2 \text{NOBr}(g) \rightarrow 2 \text{NO}(g) + \text{Br}_2(g) \). The objective is to show that the following data are consistent with a second-order reaction and determine the second-order rate constant for the reaction. *Data Presentation:* - The reaction data can be analyzed by plotting the data in three different ways. - For each plot, time \( t \) goes on the x-axis. - A zero-order reaction is linear when \([\text{NOBr}]\) is on the y-axis. - A first-order reaction is linear when \(\ln([\text{NOBr}])\) is on the y-axis. - A second-order reaction is linear when \(1/[\text{NOBr}]\) is on the y-axis. *Given Data:* \[ \begin{array}{c|cccccc} t \text{ (s)} & 0 & 5 & 10 & 15 & 50 & 85 \\ \hline [\text{NOBr}] \text{ (M)} & 0.0653 & 0.0514 & 0.0424 & 0.0361 & 0.0177 & 0.0117 \\ \end{array} \] *Questions:* 1. What is the rate law for the reaction? (Rate equations take the general form 'rate = k \cdot [A] \cdot [B]^n'.) - The reaction is determined to be second order, indicated by a linear plot of \(1/[\text{NOBr}]\) vs. time. 2. What is the value of the rate constant at the temperature of the experiment? - The rate constant \( k \) is given as 49.0. 3. What are the units for the rate law? - Options provided: - \( \text{M}^{-2} \cdot \text{s}^{-1} \) - \( \text{M}^{-3} \cdot \text{s}^{-1} \) - \( \text{M}^{-2} \cdot \text{s}^{-2} \) - \( \text{
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