In Section 18.4 we considered the following mechanism for the reaction of Br, with H;: Br2 + M 2 Br + Br + M k- Br + H2 HBr + H H + Br2 HBr + Br Although this is adequate for calculating the initial rate of reaction, before product HBr builds up, there is an additional process that can participate as the reaction continues: HBr + H H2 + Br (a) Write an expression for the rate of change of [H]. (b) Write an expression for the rate of change of [Br]. (c) As hydrogen and bromine atoms are both short-lived species, we can make the steady-state approximation and set the rates from parts (a) and (b) to 0. Express the steady-state concentrations [H] and [Br] in terms of concentrations of H, Br2, HBr, and M. [Hint: Try adding the rate for part (a) to that for part (b).] (d) Express the rate of production of HBr in terms of соncеnraions of H, Brz, HB, аnd M.

In Section 18.4 we considered the following mechanism for the reaction of Br, with H;: Br2 + M 2 Br + Br + M k- Br + H2 HBr + H H + Br2 HBr + Br Although this is adequate for calculating the initial rate of reaction, before product HBr builds up, there is an additional process that can participate as the reaction continues: HBr + H H2 + Br (a) Write an expression for the rate of change of [H]. (b) Write an expression for the rate of change of [Br]. (c) As hydrogen and bromine atoms are both short-lived species, we can make the steady-state approximation and set the rates from parts (a) and (b) to 0. Express the steady-state concentrations [H] and [Br] in terms of concentrations of H, Br2, HBr, and M. [Hint: Try adding the rate for part (a) to that for part (b).] (d) Express the rate of production of HBr in terms of соncеnraions of H, Brz, HB, аnd M.

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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For the overall gas-phase reaction of the formation of phosgene (Cl₂CO) from carbon monoxide and chlorine, the following mechanism has been proposed: Cl₂ + M2CI+M k_1 CI+CO+MCICO + M k_2 k3 CICO + Cl₂C₁₂CO+CI Derive the expected rate law assuming [M] is large and constant, and using: (a) The equilibrium assumption for the first two steps. (b) Instead using the steady state assumption for any intermediates. (c) Why does the reaction become zeroth order in [CO] in the steady state case? (d) The actual rate law is 3/2 order in [Cl₂] and first order in [CO]. Which mechanism is likely correct? (e) Is the other mechanism possible, based on the observed orders?
Please provide proper explanation of the concept and solution
Consider the following 2-step reaction mechanism, consisting of elementary steps: k1 2 XO2g) k-1 Step 1: X2O4(g) k2 Step 2: X2O4(g) + Br2७) Br2(g) + 2 XO2Br(g) a) Complete the following (if none exist, write 'none'). The reaction intermediate(s) is/are... i) The reaction catalysts(s) is/are.. b) Without assuming the relative reaction rates of Step 1 or Step 2, determine the rate law that is predicted by this mechanism. If Step 2 is a fast reaction (and Step 1 was a slow equilibrium), determine the overall reaction order.
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H2 reacts with ClF. Someone thinks this is the mechanism: H2(g) + ClF(g) → HCl(g) + HF(g) HCl(g) + ClF(g) → Cl2(g) + HF(g) (a) Write the balanced equation for the overall reaction. (b) Identify any intermediates in the mechanism, if any. (c) identify and catalysts in the mechanism, if any. (d) Write rate laws for each elementary reaction in the mechanism. (e) If the first step is slow and the second one is fast, what rate law do you expect to be observed for the overall reaction?
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Consider the hypothetical reaction A(g) + B(g) C(g) The four containers below represent this reaction being run with different initial amounts of A and B. Assume that the volume of each container is 1.0L. The reaction is second order with respect to A and first order in respect to B. Which of the containers, W,X,Y or Z, would have the greatest reaction rate? Justify your answer.
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The following mechanism has been proposed for the atmospheric decomposition of nitric oxide (NO). Step 1: 2 NO (g)  N2O Step 2: 2 (g)N2O2 (g) + H2 (g)  N2O(g) + H2O(g) Step : N2O(g) + H2 (g)  N2 (g) + H2O(g) Identify any intermediates in this reaction mechanism. Write the overall chemical reaction. Sketch the energy diagram for Step 1. E = - 4 kJ/mole. Include axes with labels. Label the reactants, product, and transition state on the energy diagram. Write the differential rate law for Step 1