Chem 113-MC02 Spring 2021 View Available Hint(s)Cl(g) + CC (g)k.→ CCL(g)(fast)ΑΣφOA chemical reaction does not occur for thisSubmitPart B Complete previous partís)Part C Complete previous part(s)Copyright 2021 Person EducanAgns vedProvide FeedbackProblemiD=16204755480ffeet-prev

A reaction may occur in multiple step. The overall reaction contain the reactants which are present…

Chapter 15 HW Exercise 15.77 - Enhanced - with Feedback and Hints artA What MISSED THIS? Read Section 15.6 (Pages 656 - 661); Watch KCV 15.6, IWE 15.9. your Consider this three-step mechanism for a reaction: Part A Ch(g) )= 2C1(g) (fast) What is the overall reaction? Figure Cl(g)+ CHC3 (g) Express your answer as a chemical eqe - HCl(g) + CCI (g) (slow). ks CCL (g) > View Available Hint(s) Cl(g) + CCls (g) (fast) AE DA chemical reaction does not occur for this

Chapter 15 HW Exercise 15.77 - Enhanced - with Feedback and Hints artA What MISSED THIS? Read Section 15.6 (Pages 656 - 661); Watch KCV 15.6, IWE 15.9. your Consider this three-step mechanism for a reaction: Part A Ch(g) )= 2C1(g) (fast) What is the overall reaction? Figure Cl(g)+ CHC3 (g) Express your answer as a chemical eqe - HCl(g) + CCI (g) (slow). ks CCL (g) > View Available Hint(s) Cl(g) + CCls (g) (fast) AE DA chemical reaction does not occur for this

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter11: Rate Of Reaction

Section: Chapter Questions

Problem 71QAP: For a certain reaction, Ea is 135 kJ and H=45 kJ. In the presence of a catalyst, the activation...

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Experiments have shown that the average frequency of chirping by a snowy tree cricket (Oecanthus fultoni) depends on temperature as shown in the table. Chirping Rate (per min) Temperature (C) 178 25.0 126 20.3 100. 17.3 What is the apparent activation energy of the process that controls the chirping? What is the rate of chirping expected at a temperature of 7.5C?
Compare the functions of homogeneous and heterogeneous catalysts.
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Experiments during a recent summer on a number of fireflies (small beetles, Lampyridaes photinus) showed that the average interval between flashes of individual insects was 16.3 s at 21.0C and 13.0 sat 27.8C. a. What is the apparent activation energy of the reaction that controls the flashing? b. What would be the average interval between flashes of an individual firefly at 30.0C? c. Compare the observed intervals and the one you calculated in part b to the rule of thumb that the Celsius temperature is 54 minus twice the interval between flashes.
Consider the following reaction: CH3X+YCH3Y+X At 25C, the following two experiments were run, yielding the following data: Experiment 1: [Y]0 = 3.0 M [CH3X] (mol/L) Time(h) 7.08 103 1.0 4.52 103 1.5 2.23 103 2.3 4.76 104 4.0 8.44 l05 5.7 2.75 l05 7.0 Experiment 2: [Y]0 = 4.5 M [CH3X] (mol/L) Time(h) 4.50 103 0 1.70 103 1.0 4.19 104 2.5 1.11 104 4.0 2.81 l05 5.5 Experiments also were run at 85C. The value of the rate constant at 85C was found to be 7.88 108 (with the time in units of hours), where [CH3X]0 = 1.0 102 M and [Y]0 = 3.0 M. a. Determine the rate law and the value of k for this reaction at 25C. b. Determine the half-life at 85C. c. Determine Ea for the reaction. d. Given that the C8X bond energy is known to be about 325 kJ/mol, suggest a mechanism that explains the results in parts a and c.
What is the difference between average rate, initial rate, and instantaneous rate?
The acid-catalyzed iodination of acetone CH3COCH3(aq) + I2(aq) CH3COCH2I(aq) + HI(aq) is a common laboratory experiment used in general chemistry courses to teach the method of initial rates. The reaction is followed spectrophotometrically by the disappearance of the color of iodine in the solution. The following data (J. P. Birk and D. L Walters, Journal of Chemical Education, Vol. 69, p. 585, 1992) were collected at 23 C for this reaction. Determine the rate law for this reaction.
For a certain reaction, Ea is 135 kJ and H=45 kJ. In the presence of a catalyst, the activation energy is 39% of that for the uncatalyzed reaction. Draw a diagram similar to Figure 11.14 but instead of showing two activated complexes (two humps) show only one activated complex (i.e., only one hump) for the reaction. What is the activation energy of the uncatalyzed reverse reaction?