Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Related questions
Question
![**Nitric Oxide Reaction Study**
**9. Study of the Reaction:**
Nitric oxide (NO) reacts with hydrogen (H₂) to form nitrous oxide (N₂O) and water (H₂O), following the chemical equation:
\[ \text{2NO}_{(g)} + \text{H}_2{_{(g)}} \rightarrow \text{N}_2\text{O}_{(g)} + \text{H}_2\text{O}_{(g)} \]
**Experimental Data:**
In a series of experiments, the initial rates of disappearance of NO were recorded as shown below.
\[
\begin{array}{|c|c|c|c|}
\hline
\text{} & \text{Initial Concentrations} & \text{} & \text{Initial Rate of Reaction} \\
\hline
\text{} & \left[\text{NO}\right] & \left[\text{H}_2\right] & \text{} \\
\hline
\text{Exp. 1} & \text{3.2 X 10}^{-3} \text{M} & \text{1.1 X 10}^{-3} \text{M} & \text{1.3 X 10}^{-5} \text{M/s} \\
\hline
\text{Exp. 2} & \text{6.4 X 10}^{-3} \text{M} & \text{1.1 X 10}^{-3} \text{M} & \text{5.2 X 10}^{-5} \text{M/s} \\
\hline
\text{Exp. 3} & \text{3.2 X 10}^{-3} \text{M} & \text{2.2 X 10}^{-3} \text{M} & \text{2.6 X 10}^{-5} \text{M/s} \\
\hline
\end{array}
\]
**Tasks:**
**a. Determination of the Rate Law Expression:**
To find the rate law expression for this reaction, analyze the changes in the initial concentrations and their corresponding rates.
**b. Identification of the Rate Law Graph:**
Three graphs are provided that represent potential rate laws with respect](https://content.bartleby.com/qna-images/question/df5aa2e5-f0b0-4839-a4ef-6f98d6dc8551/86be86c0-eef7-4890-a79e-ee3c292bfe12/b8k3ywl_processed.png)
Transcribed Image Text:**Nitric Oxide Reaction Study**
**9. Study of the Reaction:**
Nitric oxide (NO) reacts with hydrogen (H₂) to form nitrous oxide (N₂O) and water (H₂O), following the chemical equation:
\[ \text{2NO}_{(g)} + \text{H}_2{_{(g)}} \rightarrow \text{N}_2\text{O}_{(g)} + \text{H}_2\text{O}_{(g)} \]
**Experimental Data:**
In a series of experiments, the initial rates of disappearance of NO were recorded as shown below.
\[
\begin{array}{|c|c|c|c|}
\hline
\text{} & \text{Initial Concentrations} & \text{} & \text{Initial Rate of Reaction} \\
\hline
\text{} & \left[\text{NO}\right] & \left[\text{H}_2\right] & \text{} \\
\hline
\text{Exp. 1} & \text{3.2 X 10}^{-3} \text{M} & \text{1.1 X 10}^{-3} \text{M} & \text{1.3 X 10}^{-5} \text{M/s} \\
\hline
\text{Exp. 2} & \text{6.4 X 10}^{-3} \text{M} & \text{1.1 X 10}^{-3} \text{M} & \text{5.2 X 10}^{-5} \text{M/s} \\
\hline
\text{Exp. 3} & \text{3.2 X 10}^{-3} \text{M} & \text{2.2 X 10}^{-3} \text{M} & \text{2.6 X 10}^{-5} \text{M/s} \\
\hline
\end{array}
\]
**Tasks:**
**a. Determination of the Rate Law Expression:**
To find the rate law expression for this reaction, analyze the changes in the initial concentrations and their corresponding rates.
**b. Identification of the Rate Law Graph:**
Three graphs are provided that represent potential rate laws with respect
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution
Trending nowThis is a popular solution!
Step by stepSolved in 2 steps with 1 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Consider the reaction data. A products T (K) | k (s-1) 325 0.383 825 0.611 What two points should be plotted to graphically determine the activation energy of this reaction? To avoid rounding errors, use at least three significant figures in all values. X1 Yi = X2 = Y2 = Determine the rise, run, and slope of the line formed by these points. rise: run: slope: What is the activation energy of this reaction? Ea J/mol ? IIarrow_forwardConsider the base hydrolysis of an ester.RCOOR' + OH− → RCOO− + R'OH (where R and R' represent organic groups).The kinetics of this reaction, for a particular ester, were studied using the isolation method. When [OH−] << [RCOOR'] a pseudo-rate law can be posed:-d[OH-] / dt = k'' [OH-]mWith initial concentrations: [OH−]0 = 0.0015 M [RCOOR']0 = 0.700 M a plot of ln[OH-] versus t gave a straight line with slope = -0.0176 s-1 and y-intercept = -6.50.What is the order "m"?m = ? What is the corresponding pseudo rate constant k''? (include appropriate units)k'' = ?arrow_forwardCaptain Marvelibrium discovered a figure with data frorh an experiment left by Le Châtelier Flipdime. Consider the following data where A andB are mixed at initial concentrations indicated. Upon reacting the concentrations change a can be read from the plot. The reaction is A(g) + B(g) = C(g). C Time (s) Based on figure, calculate the value for Ke for the reaction. Submit Answer Tries 0/99 This discussion is closed. Send Feedback MAR 10 étv МacВос Air 000 esc F1 F2 F3 F4 F5 F6 #3 $4 3. 4 CO AB 3. Concentration (mol.dm-3)arrow_forward
- t- Assignme... Connect P Course Home E Login | Student Veri... Bb Logout MyProgrammingLab Im O KINETICS AND EQUILIBRIUM Deducing a rate law from initial reaction rate data Some measurements of the initial rate of a certain reaction are given in the table below. [-] [H.] , initial rate of reaction 1.75 M 0.767 M 16.0 M/s 7.77 M 0.767 M 71.0 M/ s 1.75 M 0.136 M 2.84 M/ s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k D k = ]arrow_forwardThe progress of a reaction is determined by various steps involving energy changes with respect to collision theory. Identify the key features of the reaction profile below. Drag the appropriate labels to their respective targets in the energy profile diagram.arrow_forwardFor a chemical reaction, the rate constant at 233.9 °C is 0.00306 s^-1, and the activation energy is 24.27 kJ mol^-1. Calculate the value of the rate constant at 326.7 °C. Report answer with 5 places past the demical point.arrow_forward
arrow_back_ios
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
ChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill Education
Principles of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning 
Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill Education
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY