Suppose the decomposition of nitrogen dioxide proceeds by the following mechanism: step elementary reaction 1 NO₂(9) NO(g) + O(g) k₁ 2 O(g) + NO₂(g) → O₂(g) + NO(g) k₂ Suppose also k₁k₂. That is, the first step is much faster than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally observable rate law for the overall chemical reaction. Note: your answer should not contain the i concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k₁, k₂, and (if necessary) the rate constants k.₁ and k₂ for the reverse of the two elementary reactions in the mechanism. 0 rate= - 0 k= *0 rate constant 0-0 Do 00 X 5 ?

Suppose the decomposition of nitrogen dioxide proceeds by the following mechanism: step elementary reaction 1 NO₂(9) NO(g) + O(g) k₁ 2 O(g) + NO₂(g) → O₂(g) + NO(g) k₂ Suppose also k₁k₂. That is, the first step is much faster than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally observable rate law for the overall chemical reaction. Note: your answer should not contain the i concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k₁, k₂, and (if necessary) the rate constants k.₁ and k₂ for the reverse of the two elementary reactions in the mechanism. 0 rate= - 0 k= *0 rate constant 0-0 Do 00 X 5 ?

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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