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4:00 Step 1 Step 2 Question 10 of 13 H₂(g) + 2NO(g) → N₂O(g) + H₂O(g) (slow) N₂O(g) + H₂(g) → N₂(g) + H₂O(g) (fast) A) rate= K[H₂] [NO] B) rate = k[H₂]²[NO] rate = = K[H₂] [NO]² D) rate= = K[H₂]²[NO]² Submit rate = K[H₂] [N₂O] Learn More in OpenStax Periodic Table

4:00 Step 1 Step 2 Question 10 of 13 H₂(g) + 2NO(g) → N₂O(g) + H₂O(g) (slow) N₂O(g) + H₂(g) → N₂(g) + H₂O(g) (fast) A) rate= K[H₂] [NO] B) rate = k[H₂]²[NO] rate = = K[H₂] [NO]² D) rate= = K[H₂]²[NO]² Submit rate = K[H₂] [N₂O] Learn More in OpenStax Periodic Table

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter11: Chemical Kinetics
Section: Chapter Questions
Problem 11.63PAE: The following mechanism is proposed for a reaction: NO + Br2 —* NOBr2 (slow) NOBr2 + NO —»2 NOBr...
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4:00 Step 1 Step 2 Question 10 of 13 H₂(g) + 2NO(g) → N₂O(g) + H₂O(g) (slow) N₂O(g) + H₂(g) → N₂(g) + H₂O(g) (fast) A) rate= K[H₂] [NO] B) rate = k[H₂]²[NO] rate = = K[H₂] [NO]² D) rate= = K[H₂]²[NO]² Submit rate = K[H₂] [N₂O] Learn More in OpenStax Periodic Table
Transcribed Image Text:4:00 Step 1 Step 2 Question 10 of 13 H₂(g) + 2NO(g) → N₂O(g) + H₂O(g) (slow) N₂O(g) + H₂(g) → N₂(g) + H₂O(g) (fast) A) rate= K[H₂] [NO] B) rate = k[H₂]²[NO] rate = = K[H₂] [NO]² D) rate= = K[H₂]²[NO]² Submit rate = K[H₂] [N₂O] Learn More in OpenStax Periodic Table
4:00 What is the rate law for the proposed mechanism? Step 1 Question 10 of 13 Step 2 H₂(g) + 2NO(g) N₂O(g) + H₂O(g) (slow) N₂O(g) + H₂(g) → N₂(g) + H₂O(g) (fast) A) rate = = K[H₂] [NO] B) rate = K[H₂]²[NO] Submit C) rate = K[H₂] [NO]² LEL 12 NO12 Tap here or pull up for additional resources
Transcribed Image Text:4:00 What is the rate law for the proposed mechanism? Step 1 Question 10 of 13 Step 2 H₂(g) + 2NO(g) N₂O(g) + H₂O(g) (slow) N₂O(g) + H₂(g) → N₂(g) + H₂O(g) (fast) A) rate = = K[H₂] [NO] B) rate = K[H₂]²[NO] Submit C) rate = K[H₂] [NO]² LEL 12 NO12 Tap here or pull up for additional resources
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