**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{

In order to find the order of the reaction, we have to plot 3 different graphs. The graph having the…

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

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

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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