E17E.1(a) The reaction mechanism for the decomposition of A2 is thought to be A₂ A+A k₁₂ kb A+B → P where the dissociation of A2 is first order in A2, and the recombination of A is second order in A; the reaction of A with B is first order in both A and B. Deduce the rate law for the rate of formation of P in two ways: (i) by assuming a pre-equilibrium between A2 and A, and (ii) by assuming that the steady- state approximation can be applied to A.

E17E.1(a) The reaction mechanism for the decomposition of A2 is thought to be A₂ A+A k₁₂ kb A+B → P where the dissociation of A2 is first order in A2, and the recombination of A is second order in A; the reaction of A with B is first order in both A and B. Deduce the rate law for the rate of formation of P in two ways: (i) by assuming a pre-equilibrium between A2 and A, and (ii) by assuming that the steady- state approximation can be applied to A.

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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E17E.1(a) The reaction mechanism for the decomposition of A, is thought to be A, A+A A+B - where the dissociation of A, is first order in A, and the recombination of A is second order in A; the reaction of A with B is first order in both A and B. Deduce the rate law for the rate of formation of P in two ways: (i) by assuming a pre-equilibrium between A, and A, and (ii) by assuming that the steady- state approximation can be applied to A.
The acid-catalyzed hydrolysis of sucrose occurs by the fol-lowing overall reaction whose kinetic data are given below:C₁₂H₂₂O₁₁(s) H₂O(l) →C₆H₁₂O₆(aq) C₆H₁₂O₆(aq) (a) Determine the rate constant and the half-life of the reaction.(b) How long does it take to hydrolyze 75% of the sucrose?(c) Other studies have shown that this reaction is actually sec-ond order overall but appears to follow first-order kinetics.(Such a reaction is called a pseudo–first-order reaction.) Sug-gest a reason for this apparent first-order behavior.
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Define the following terms :(a) Pseudo first order reaction.(b) Half life period of reaction (t1/2).
E17B.1(b) In a study of the enzyme-catalysed oxidation of ethanol, the molar concentration of ethanol decreased in a first-order reaction from 220 mmol dm3 to 56.0 mmol dm in 1.22 x 10 s. What is the rate constant of the reaction?
(1) The gas phase decomposition of dinitrogen pentoxide at 335 KN2O5(g)2 NO2(g) + ½ O2(g)is first order in N2O5 with a rate constant of 4.70×10-3 s-1.If the initial concentration of N2O5 is 3.97×10-2 M, the concentration of N2O5 will be 8.22×10-3 M after ______s have passed. (1b) The gas phase decomposition of sulfuryl chloride at 600 K SO2Cl2(g) SO2(g) + Cl2(g) is first order in SO2Cl2 with a rate constant of 2.80×10-3 min-1. If the initial concentration of SO2Cl2 is 4.90×10-3 M, the concentration of SO2Cl2 will be M after ______ 499 min have passed.
E17B.4(a) The second- order rate constant for the reaction CH,COOCH. (aa OH (aq)CH, CO,(aq) + CH,CH2OH ( aq) is 0.11 dm mois.What is the concentration of ester (CH,COOC,H) after (i) 20 s, (ii) 15 min when ethyl ethanoate is added to aqueous sodium hydroxide so that the initial concentrations are [NaOH] 0.060 mol dm and [CH,COOC,H,] = 0.110 mol dm3? re ed -3 3 AL2R C +D ation
E17B.3(b) The rate constant for the first-order decomposition of a compound A in the reaction 2 A-> P is k, = 3.56 x 10 s at 25°C. What is the half-life of A? If the initial partial pressure of A is 33.0 kPa, what will be its partial pressure (i) 50 s, (ii) 20 min after initiation of the reaction? 1 91
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E17E.2(a) The following mechanism has been proposed for the decomposition of ozone in the atmosphere: 03 → 0₂+0 k₁ O₁₂+0 → 03 K →> 2 k₁ Show that if the third step is rate limiting, then the rate law for the decomposition of O3 is second-order in O3 and of order −1 in O̟.
The reaction mechanismA2 = A+A (fast)A+ B → P (slow)involves an intermediate A. Deduce the rate law for the formation of P.
A second-order-reaction of the type A +2 B→ P was carried out in a solution that was initially 0.075 mol dm3 in A and 0.030 mol dm3 in B. After 1.0 h the concentration of A had fallen to 0.045 mol dm3. (a) Calculate the rate constant. (b) What is the half-life of the reactants? The rate constant for the decomposition of a certain substance is 1.70 x 10-2 dm³ mol-¹ s¹ at 24°C and 2.01 x 10-2 dm³ mol-¹ s¹ at 37°C. Evaluate the Arrhenius parameters of the reaction. A reaction 2 AP has a third-order rate law with k = 3.50 x 104 dmº mol2 s¹. Calculate the time required for the concentration of A to change from 0.077 mol dm3 to 0.021 mol dm³.