7. Let's consider the reaction: 2 NO(g) + 2 H2(g) - a) Explain why this reaction is unlikely to be an elementary step. b) A proposed mechanism is: 2 H20(g) + N2(g) Step 1: 2 NO(g) = N2O2(g) fast forward (kı) and reverse (k-1) Step 2: N2O2(g) + H2(g) → N2(g) + H2O2(g) slow (k2) Step 3: H2O2(g) + H2(g) → 2 H2O(g) fast (k3) Using this mechanism, determine the rate law of the reaction as a function of [NO] and [H2]. c) Express the rate constant of the reaction as a function of the rate constants of the elementary steps: kı, k.1, k2, and k3.
7. Let's consider the reaction: 2 NO(g) + 2 H2(g) - a) Explain why this reaction is unlikely to be an elementary step. b) A proposed mechanism is: 2 H20(g) + N2(g) Step 1: 2 NO(g) = N2O2(g) fast forward (kı) and reverse (k-1) Step 2: N2O2(g) + H2(g) → N2(g) + H2O2(g) slow (k2) Step 3: H2O2(g) + H2(g) → 2 H2O(g) fast (k3) Using this mechanism, determine the rate law of the reaction as a function of [NO] and [H2]. c) Express the rate constant of the reaction as a function of the rate constants of the elementary steps: kı, k.1, k2, and k3.
Introduction to General, Organic and Biochemistry
11th Edition
ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Chapter7: Reaction Rates And Chemical Equilibrium
Section: Chapter Questions
Problem 7.65P
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