   Chapter 15, Problem 32GQ

Chapter
Section
Textbook Problem

The equilibrium constant for the reactionN2(g) + O2(g) ⇄ 2 NO(g)is 1.7 × 10−3 at 2300 K. (a) What is K for the reaction when written as follows? ½ N2(g) + ½ O2(g) ⇄ NO(g) (b) What is K for the following reaction? 2 NO(g) ⇄ N2(g) + O2(g)

(a)

Interpretation Introduction

Interpretation: The equilibrium constant of the given reactions has to be determined.

Concept introduction:

Equilibrium constant: It is the ratio of products to reactants has a constant value when the reaction is in equilibrium at a certain temperature. And it is represented by the letter K.

For a reaction,

aA+bBcC+dD

The equilibrium constant is, K=[C]c[D]d[A]a[B]b

Where, a, b, c and d are the stoichiometric coefficients of reactant and product in the reactions.

Explanation

Given,

The balanced chemical equation for the given reaction is,

N2(g)+O2(g)2NO(g)

The equilibrium constant, K1 for the reaction is,

K1=[NO]2[N2][O2] =1.7×103

The balanced equation for the reaction (a) is,

12N2(g)+12O2(g)NO(g)

The equilibrium constant, <

(b)

Interpretation Introduction

Interpretation: The equilibrium constant of the given reactions has to be determined.

Concept introduction:

Equilibrium constant: It is the ratio of products to reactants has a constant value when the reaction is in equilibrium at a certain temperature. And it is represented by the letter K.

For a reaction,

aA+bBcC+dD

The equilibrium constant is, K=[C]c[D]d[A]a[B]b

Where, a, b, c and d are the stoichiometric coefficients of reactant and product in the reactions.

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