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2 NO₂(g) + F2(g) → NO₂F(g) AH = -284 kJ/mol, NO₂(g) and F₂ (g) can react to produce NO₂F(g), as represented above. A proposed mechanism for the reaction has two elementary steps, as shown below. Step 1: NO₂+ F2 NO₂F+F (slow) Step 2: NO₂+ F NO₂F (fast) (a) Write a rate law for the overall reaction that is consistent with the proposed mechanism.

2 NO₂(g) + F2(g) → NO₂F(g) AH = -284 kJ/mol, NO₂(g) and F₂ (g) can react to produce NO₂F(g), as represented above. A proposed mechanism for the reaction has two elementary steps, as shown below. Step 1: NO₂+ F2 NO₂F+F (slow) Step 2: NO₂+ F NO₂F (fast) (a) Write a rate law for the overall reaction that is consistent with the proposed mechanism.

Chemistry: Matter and Change
Chemistry: Matter and Change
1st Edition
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Chapter16: Reaction Rates
Section: Chapter Questions
Problem 70A
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Step 2: NO₂(g) and F₂ (g) can react to produce NO₂F(g), as represented above. A proposed mechanism for the reaction has two elementary steps, as shown below. Step 1: NO₂+ F₂ → NO₂F+F (slow) NO₂+ F→ NO₂F BIU (a) Write a rate law for the overall reaction that is consistent with the proposed mechanism. X² X₂ C Ω (fast) !!! 2 NO₂(g) + F₂(g) → NO₂F(g) AH = -284 kJ/mol, III E TIN
Transcribed Image Text:Step 2: NO₂(g) and F₂ (g) can react to produce NO₂F(g), as represented above. A proposed mechanism for the reaction has two elementary steps, as shown below. Step 1: NO₂+ F₂ → NO₂F+F (slow) NO₂+ F→ NO₂F BIU (a) Write a rate law for the overall reaction that is consistent with the proposed mechanism. X² X₂ C Ω (fast) !!! 2 NO₂(g) + F₂(g) → NO₂F(g) AH = -284 kJ/mol, III E TIN
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