2NO2(g)+F2(g)→NO2F(g)ΔH∘rxn=−284kJ/molrxnNO2(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.

Answered: 2NO2(g)+F2(g)→NO2F(g)ΔH∘rxn=−284kJ/molr…

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter8: Reaction Rates And Equilibrium

Section: Chapter Questions

Problem 8.28E

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2NO2(g)+F2(g)→NO2F(g)ΔH∘rxn=−284kJ/molrxn

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.

Expert Solution

Step 1

The rate law of a reaction is determined experimentally by measuring the rate of reaction. In rate law, the sum of the power of the concentration term is known as the order of the reaction.

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