Remaining Time: 2 hours, 22 minutes, 53 seconds.Question Completion Status:Below is the initial rate data from a few experiments on the reaction:A+B> Products.[A]; (M)Experiment #11123The reaction is first order in A. The rate constant is thus:O 5.656 Ms-1O 2.828 M-1-1O 11.31 s-1O 1.414 M-25-11.002.002.00QUESTION 7Consider the following reaction:O Equal to the rate of reaction.O Three times the rate of reactionO Twice the rate of reactionOne third of the rate of reaction[B]; (M)2 03(g) -> 3 O2(g)What is the rate of consumption of O3 compared to the rate of reaction?O Half of the rate of reaction.1.00.002.00Click Save and Submit to save and submit. Click Save All Answers to save all answers.Rate; (M s-1)1.4142.82811.31İyS

Answered: Image /qna-images/answer/e9307869-8236-4dd7-a271-3115af971e88.jpg

Remaining Time: 2 hours, 22 minutes, 53 seconds. Question Completion Status: Below is the initial rate data from a few experiments on the reaction: A+B> Products. [A]; (M) Experiment # 12 3 The reaction is first order in A. The rate constant is thus: O 5.656 Ms-1 © 2.828 M-1s-1 O 11.31 s-1 1.414 M-2-1 1.00 2.00 2.00 QUESTION 7 Consider the following reaction: [B]; (M) O Equal to the rate of reaction O Three times the rate of reaction OTwice the rate of reaction One third of the rate of reaction. O Half of the rate of reaction 1.00 1.00 2.00 2 03(g) -> 3 O2(g) What is the rate of consumption of O3 compared to the rate of reaction? Click Save and Submit to save and submit. Click Save All Answers to save all answers. Rate; (M s-1) 1.414 2.828 11.31

Remaining Time: 2 hours, 22 minutes, 53 seconds. Question Completion Status: Below is the initial rate data from a few experiments on the reaction: A+B> Products. [A]; (M) Experiment # 12 3 The reaction is first order in A. The rate constant is thus: O 5.656 Ms-1 © 2.828 M-1s-1 O 11.31 s-1 1.414 M-2-1 1.00 2.00 2.00 QUESTION 7 Consider the following reaction: [B]; (M) O Equal to the rate of reaction O Three times the rate of reaction OTwice the rate of reaction One third of the rate of reaction. O Half of the rate of reaction 1.00 1.00 2.00 2 03(g) -> 3 O2(g) What is the rate of consumption of O3 compared to the rate of reaction? Click Save and Submit to save and submit. Click Save All Answers to save all answers. Rate; (M s-1) 1.414 2.828 11.31

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 98CWP: A certain reaction has the form aAProducts At a particular temperature, concentration versus time...

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The hypothetical reaction QR+Xproductswas monitored at 27C as a function of time. The following plots are obtained: (a) Write the rate expression for the reaction. (b) What is the rate constant if the rate of the reaction is 0.29 mol/L min when [ QR ]=[ X ]=1.000M? (c) What is the half-life for the consumption of QR when [ QR ]=0.0866M? (d) If the initial concentration of [ X ]=5.00M, what is [ X ] after 4.7 min?
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For the reaction QW+X, the following data were obtained at 30 C: [Q]initial (M) 0.170 0.212 0.357 Rate(mol/L/s) 6.68103 1.04102 2.94102 (a) What is the order of the reaction with respect to [Q], and what is the rate equation? (b) What is the rate constant?
A certain reaction has the form aAProducts At a particular temperature, concentration versus time data were collected. A plot of 1/ [A] versus Lime (in seconds) gave a straight line with a slope of 6.90 102. What is the differential rate law for this reaction? What is the integrated rate law for this reaction? What is the value of the rate constant for this reaction? If [A]0 for this reaction is 0.100 M, what is the first half-life (in seconds)? If the original concentration (at t = 0) is 0.100 M, what is the second half-life (in seconds)?
When formic acid is heated, it decomposes to hydrogen and carbon dioxide in a first-order decay: HCOOH(g)CO2(g)+H2(g) The rate of reaction is monitored by measuring the total pressure in the reaction container. Time (s) Pressure (torr) 0 220 50 324 100 379 150 408 200 423 250 431 300 435 Calculate the rate constant and half-life in seconds for the reaction. At the start of the reaction (time = 0), only formic acid is present. (HINT: Find the partial pressure of formic acid using Dalton's law of partial pressure and the reaction stoichiometry to find PHCOOH at each time.)
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