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Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

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BuyFindarrow_forward

Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

Nitrogen monoxide is reduced by hydrogen to give nitrogen and water:

2 NO(g) + 2 H2(g) → N2(g) + 2 H2O(g)

One possible mechanism for this reaction involves the following reactions:

2 NO(g) → N2O2(g)

N2O2(g) + H2(g) → N2O(g) + H2O(g)

N2O(g) + H2(g) → N2(g) + H2O(g)

What is the molecularity of each of the three steps? What is the rate equation for the third step? Identify the intermediates in this reaction; how many different intermediates are there? Show that the sum of these elementary steps gives the equation for the overall reaction.

Interpretation Introduction

Interpretation: The molecularity, rate equation, and overall reaction has to be given.

Concept introduction:

Molecularity of the reaction is the number of molecules that is seen on the reactant side of an elementary reaction.

The reaction that involves in one reactant molecule is unimolecular reaction.

The reaction that involves in two reactant molecules is bimolecular reaction.

The reaction that involves in three reactant molecules is termolecular reaction.

Rate equations for elementary steps:

The rate equation for elementary step is defined by its reaction stoichiometry.

  Elementarystep:AProduct.Rateequation:Rate=k[A]

Explanation

The molecularity of the reaction is ,

Molecularity of elementary steps:

  Step1:2NO(g)N2O2(g) Step2:N2O2(g) + H2(g)N2O(g) + H2O(g)Step3:    N2O(g)  + H2(g)N2(g)+H2O(g)

In all the three elementary steps, two molecules are involved, which says all the steps are bimolecular.

Rate of elementary steps:

  Step1:2NO(g)N2O2(g) Step2:N2O2(g) + H2(g)N2O(g) + H2O(g)Step3:    N2O(g)  + H2(g)N2(g)+H2O(g)Rate1:Rate=k[NO]2Rate2:Rate=k[N2O2][H2]Rate3:Rate=k[N2O][H2]

The rate equation for elementary step is defined by its reaction stoichiometry

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