Step 1Step 2What is the rate law for the proposed mechanism?H₂(g) + 2NO(g) N₂O(g) + H₂O(g)(slow)4N₂O(g) + H₂(g) → N₂(g) + H₂O(g)(fast)A) rate k[H₂][NO]B) rate= K[H₂]³[NO]C) rate= K[H₂][NO].D) rate= K[H₂][NO]E) rate k[H₂][N₂O]=

The rate law of a reaction is determined by the slow step of a reaction. Since slow step is the rate…

Step 1 Step 2 What is the rate law for the proposed mechanism? H₂(g) + 2NO(g) N₂O(g) + H₂O(g) (slow) 4 N₂O(g) + H2(g) → N₂(g) + H₂O(g) (fast) A) rate k[H₂][NO] B) rate= K[H₂][NO] C) rate = K[H₂][NO] D) rate= K[H₂][NO] E) rate= k[H₂][N₂O] 20

Step 1 Step 2 What is the rate law for the proposed mechanism? H₂(g) + 2NO(g) N₂O(g) + H₂O(g) (slow) 4 N₂O(g) + H2(g) → N₂(g) + H₂O(g) (fast) A) rate k[H₂][NO] B) rate= K[H₂][NO] C) rate = K[H₂][NO] D) rate= K[H₂][NO] E) rate= k[H₂][N₂O] 20

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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Question

Step 1
Step 2
What is the rate law for the proposed mechanism?
H₂(g) + 2NO(g) N₂O(g) + H₂O(g)
(slow)
4
N₂O(g) + H₂(g) → N₂(g) + H₂O(g)
(fast)
A) rate k[H₂][NO]
B) rate= K[H₂]³[NO]
C) rate= K[H₂][NO].
D) rate= K[H₂][NO]
E) rate k[H₂][N₂O]
=

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