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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E17C.1(b) The equilibrium constant for the binding of a drug molecule to a protein was measured as 200. In a separate experiment, the rate constant for the binding process, which is second order overall, was found to be 1.5 x 10 dm mol s. What is the rate constant for the first-order dissociation of the drug molecule from the protein- drug complex?
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.
20B.2(b) The rate constant for the first-order decomposition of a compound A in the reaction 2 A→P is krr=3.56×10−7 s−1 at 25 °C. What is the half-life of A? What will be the pressure, initially 33.0 kPa after (i) 50 s, (ii) 20 min after initiation of the reaction?
23.1b On the basis of the following proposed mechanism, account for the experimental fact that the rate law for the decomposition 2 N₂O5(g) → 4 NO₂(g) + O₂(g) is v=k[N₂O5]. (1) N₂O5NO2 + NO3 (2) NO₂ + NO3 → NO₂ + O₂ + NO (3) NO+N₂O5 → NO₂ + NO₂+NO₂ 23.2a A slightly different mechanism for the decomposition of N₂O5 from that in Exercise 23.1b has also been proposed. It differs only in the last step, which is replaced by (3) NO+NO3 →→ NO₂+NO₂ k3 Show that this mechanism leads to the same overall rate law. k₁, k₁ k₂ k3 23.2b Consider the following mechanism for the thermal decomposition of R₂: (1) R₂ → R+R (2) R+ R₂ → PB+R' (3) R' → PA+R (4) R+R PA + PB where R₂, PA, PB are stable hydrocarbons and R and R' are radicals. Find the dependence of the rate of decomposition of R₂ on the concentration of R₂. 16
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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