A reaction has the following proposed mechanism: A2(g) + B(s)-> A₂B(s) (fast) A2B(s)-> A(g) + AB(s) (slow) AB(s) + C(g) -> AC(g) + B(s) (fast) A(g) + C(g) -> AC(g)(fast) For this mechanism, the species B would best be classified as a(n) heterogeneous catalyst homogeneous catalyst intermediate transition state structure product of the overall reaction

A reaction has the following proposed mechanism: A2(g) + B(s)-> A₂B(s) (fast) A2B(s)-> A(g) + AB(s) (slow) AB(s) + C(g) -> AC(g) + B(s) (fast) A(g) + C(g) -> AC(g)(fast) For this mechanism, the species B would best be classified as a(n) heterogeneous catalyst homogeneous catalyst intermediate transition state structure product of the overall reaction

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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What is the rate order with respect to the substances in the overyrate law given: A + B -> C(slow) A + C -> 3 D (fast)
Recall the reaction in lecture slides #42 and #43: 2 NO2Cl(g) --> 2 NO2(g) + Cl2(g). The proposed mechanism from that example is below. (1) NO2Cl(g) --> NO2(g) + Cl(g)(2) NO2Cl(g) + Cl(g) --> NO2(g) + Cl2(g) If step (1) is the rate-determining step for the reaction, what is the reaction rate law? Group of answer choices rate = k [NO2Cl] rate = k [NO2Cl]2 rate = k [NO2Cl][Cl] rate = k [NO2Cl]2 [NO2]2 [Cl2] There is not enough information provided to predict the rate law.
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2. Imagine you run a reaction whose free energy of activation (AG*) is 18 kcal/mol. If it were a first order reaction, its’ half life (the time for half the starting material to go away) or half the product to form (assuming a 100% yield) would by In2/k where k is the rate constant. How long will it take for the reaction to be done if you run the reaction in an ice-salt bath at room temperature (20 °C) if the rate constant were 1 x 104/sec?
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For the reaction 2NO + Cl2 ---> 2NOCl Match the appropriate rate law to each postulated mechanism. A Rate = k[NO]2[Cl2] B Rate = k[Cl2] C Rate = k[NO]2[Cl2]2 D Rate = k[Cl2]2 E Rate = k[NO] F Rate = k[NO][Cl2]2 G Rate = k[NO]2 H Rate = k[NO][Cl2] I None of the above NO + Cl2 NOCl2 fast equilibriumNOCl2 + NO 2NOCl slow 2NO N2O2 fast equilibriumN2O2 + Cl2 2NOCl slow Cl2 2Cl slowCl + NO NOCl fast NO + Cl2 NOCl + Cl slowCl + NO NOCl fast
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Q2) Consider the following third order reaction: A➜ product The following is the integrated rate law for the third order reaction: 2[A];² 11/2 = kt + 1.5 K[A]0² 2[A]o² If the concentration of the reactant after 26.5 second of the experiment was found to 0.348 M and the rate constant for this reaction was found to be 1.5x10¹² M².S¹. a) Determine the initial concentration of the reactant. b) What is the half-life of this reaction? c) What is the concentration of the reactants after 1.00 min of the experiment?
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