Problem: The rate law for the reaction 2 H₂ (g) + 2 NO (g)→ N₂ (g) + 2 H₂O (g) is observed to berate = k[NO]²[H₂]. Three possible mechanisms have been proposed; which can be ruled out?Proposed Mechanism I:NO (g) + H₂(g) →→→ H₂O (g) + N (g) [slow]N (g) + NO (g) → N₂ (g) + 0 (g) [fast]H₂O (g) [fast]2O(g) + H₂(g) →Proposed Mechanism II:2 NO(g) + H₂(g) → N₂0 (g) + H₂O (g) [slow]N₂O(g) + H₂(g) → N₂ (g) + H₂O (g) [fast]Proposed Mechanism III:2 NO (g) = N₂O₂ (g) [fast equilibrium]N₂O₂(g) + H₂(g) → N₂0 (g) + H₂O (g) [fast]N₂O(g) + H₂(g) → N₂ (g) + H₂O (g) [fast]

Rate law: The rate law describes how the rate of a chemical reaction depends on the reactant…

Problem: The rate law for the reaction 2 H₂ (g) + 2 NO (g)→ N₂ (g) + 2 H₂O (g) is observed to be rate = K[NO]²[H₂]. Three possible mechanisms have been proposed; which can be ruled out? Proposed Mechanism l: NO (g) + H₂(g) → H₂O (g) + N (g) [slow] N (g) + NO (g) →→→ N₂ (g) + 0 (g) [fast] O (g) + H₂ (g) → H₂O (g) [fast] Proposed Mechanism II: 2 NO (g) + H₂(g) → N₂O (g) + H₂O (g) [slow] N₂O(g) + H₂(g) →→→ N₂ (g) + H₂O (g) [fast] Proposed Mechanism III: 2 NO (g) = N₂O₂ (g) [fast equilibrium] N₂O₂ (g) + H₂(g) → N₂0 (g) + H₂O (g) [fast] N₂O (g) + H₂ (g) → N₂ (g) + H₂O (g) [fast]

Problem: The rate law for the reaction 2 H₂ (g) + 2 NO (g)→ N₂ (g) + 2 H₂O (g) is observed to be rate = K[NO]²[H₂]. Three possible mechanisms have been proposed; which can be ruled out? Proposed Mechanism l: NO (g) + H₂(g) → H₂O (g) + N (g) [slow] N (g) + NO (g) →→→ N₂ (g) + 0 (g) [fast] O (g) + H₂ (g) → H₂O (g) [fast] Proposed Mechanism II: 2 NO (g) + H₂(g) → N₂O (g) + H₂O (g) [slow] N₂O(g) + H₂(g) →→→ N₂ (g) + H₂O (g) [fast] Proposed Mechanism III: 2 NO (g) = N₂O₂ (g) [fast equilibrium] N₂O₂ (g) + H₂(g) → N₂0 (g) + H₂O (g) [fast] N₂O (g) + H₂ (g) → N₂ (g) + H₂O (g) [fast]

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 reaction 2NO + Cl2 ---> 2NOCl Match the appropriate rate law to each postulated mechanism. A Rate = k[NO]2[Cl2] B Rate = k[Cl2] C Rate = k[NO]2[Cl2]2 D Rate = k[Cl2]2 E Rate = k[NO] F Rate = k[NO][Cl2]2 G Rate = k[NO]2 H Rate = k[NO][Cl2] I None of the above NO + Cl2 NOCl2 fast equilibriumNOCl2 + NO 2NOCl slow 2NO N2O2 fast equilibriumN2O2 + Cl2 2NOCl slow Cl2 2Cl slowCl + NO NOCl fast NO + Cl2 NOCl + Cl slowCl + NO NOCl fast
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Consider the rate law, (Look at picture) The balanced equation corresponding to this rate law is: Group of answer choices 1/2 CH4 + O2 → H2O + 1/2 CO2 CH4 + 2 O2 → 2 H2O + CO2 CH4 + CO2 → 2H2O + O2 CH4 + O2 → H2O + CO2 CH4 + O2 → H2O + CO2