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Suppose the formation of nitrogen dioxide proceeds by the following mechanism: elementary reaction rate constant 2 NO(g) N₂O₂(9) k₁ N₂O₂(g) + O₂(9) k₂ Suppose also k₁ «k₂. That is, the first step is much slower than the second. step 1 2 - 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 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 k-2 for the reverse of the two elementary reactions in the mechanism. 2 NO₂(g) 0 rate = k k = 0

Suppose the formation of nitrogen dioxide proceeds by the following mechanism: elementary reaction rate constant 2 NO(g) N₂O₂(9) k₁ N₂O₂(g) + O₂(9) k₂ Suppose also k₁ «k₂. That is, the first step is much slower than the second. step 1 2 - 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 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 k-2 for the reverse of the two elementary reactions in the mechanism. 2 NO₂(g) 0 rate = k k = 0

Physical Chemistry
Physical Chemistry
2nd Edition
ISBN:9781133958437
Author:Ball, David W. (david Warren), BAER, Tomas
Publisher:Ball, David W. (david Warren), BAER, Tomas
Chapter5: Introduction To Chemical Equilibrium
Section: Chapter Questions
Problem 5.12E: 5.12. True or false: If all the partial pressures of reactants and products drop by half, the value...
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Suppose the formation of nitrogen dioxide proceeds by the following mechanism: elementary reaction 2 NO(g) N₂O₂(9) N₂O₂(g) + O₂(g) → 2NO₂(g) step 1 2 Write the balanced chemical equation for the overall chemical reaction: Suppose also k₁ <<k₂. That is, the first step is much slower than the second. Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the 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 k-2 for the reverse of the two elementary reactions in the mechanism. 0 rate = k k - 0 rate constant = k₁ k₂ ロ→ロ 00 X S
Transcribed Image Text:Suppose the formation of nitrogen dioxide proceeds by the following mechanism: elementary reaction 2 NO(g) N₂O₂(9) N₂O₂(g) + O₂(g) → 2NO₂(g) step 1 2 Write the balanced chemical equation for the overall chemical reaction: Suppose also k₁ <<k₂. That is, the first step is much slower than the second. Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the 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 k-2 for the reverse of the two elementary reactions in the mechanism. 0 rate = k k - 0 rate constant = k₁ k₂ ロ→ロ 00 X S
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