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The reaction of hydrogen and bromine, H2(g) + Br2(g) → 2 HBr(g). occurs through a radical mechanism. The individual steps may be written asBr2 → Br + Br kaBr+H2 → H+HBr kbH + Br2 →  Br+ HBr kcH + HBr → H2 + Br kdBr + Br + M → Br2 + M ka(a) Deduce the expressions for the steady-state concentrations [Br] and [H] from the expressions for the net rates of formation of H and Br. (b) By combining these expressions, show that the rate of formation of HBr is 2kb(ka/ko)' 1/2 [H2] [Br2] 3/2/{[Br2] + (kd/ko)}. (c) What are the orders of the reaction (with respect to each species) when the concentration of H Bris (i) very low, (ii) very high? Suggest an interpretation in each case.

The reaction of hydrogen and bromine, H2(g) + Br2(g) → 2 HBr(g). occurs through a radical mechanism. The individual steps may be written asBr2 → Br + Br kaBr+H2 → H+HBr kbH + Br2 →  Br+ HBr kcH + HBr → H2 + Br kdBr + Br + M → Br2 + M ka(a) Deduce the expressions for the steady-state concentrations [Br] and [H] from the expressions for the net rates of formation of H and Br. (b) By combining these expressions, show that the rate of formation of HBr is 2kb(ka/ko)' 1/2 [H2] [Br2] 3/2/{[Br2] + (kd/ko)}. (c) What are the orders of the reaction (with respect to each species) when the concentration of H Bris (i) very low, (ii) very high? Suggest an interpretation in each case.

Chemistry
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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The reaction of hydrogen and bromine, H2(g) + Br2(g) → 2 HBr(g). occurs through a radical mechanism. The individual steps may be written as
Br2 → Br + Br ka
Br+H2 → H+HBr kb
H + Br2 →  Br+ HBr kc
H + HBr → H2 + Br kd
Br + Br + M → Br2 + M ka
(a) Deduce the expressions for the steady-state concentrations [Br] and [H] from the expressions for the net rates of formation of H and Br. (b) By combining these expressions, show that the rate of formation of HBr is 2kb(ka/ko)' 1/2 [H2] [Br2] 3/2/{[Br2] + (kd/ko)}. (c) What are the orders of the reaction (with respect to each species) when the concentration of H Br
is (i) very low, (ii) very high? Suggest an interpretation in each case.

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