Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Chapter 13, Problem 27E

At a given temperature, K = 1.3 × 10−2 for the reaction

N 2 ( g ) + 3 H 2 ( g ) 2 NH 3 ( g )

Calculate values of K for the following reactions at this temperature.

a 1 2 N 2 ( g ) + 3 2 H 2 ( g ) NH 3 ( g )

b. 2 N H 3 ( g ) N 2 ( g ) + 3 H ( g )

c. NH 3 ( g ) 1 2 N 2 ( g ) + 3 2 H 2 ( g )

d. 2N 2 ( g ) + 6 H 2 ( g ) 4 NH 3 ( g )

(a)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The equilibrium constant (K) for each of the given gas-phase reactions is to be stated.

Concept introduction: The state when the reactants involved in a chemical reaction and the products formed in the reaction exist in concentrations having no further tendency to change is known as an equilibrium state of the reaction. When the equilibrium constant is expressed in terms of concentration, it is represented K .

To determine: The equilibrium constant for the given reaction.

Answer to Problem 27E

Answer

The equilibrium constant for the given reaction is 0.11_ .

Explanation of Solution

Given

The stated reaction is,

N2(g)+3H2(g)2NH3(g)

The equilibrium constant (K) for the stated reaction is 1.3×102 .

At equilibrium, the equilibrium constant expression is stated,

K=[NH3]2[N2][H2]3

Where,

  • K is the equilibrium constant.

The stated reaction is,

12N2(g)+32H2(g)NH3(g)

At equilibrium, the equilibrium constant expression is stated,

K1=[NH3][N2]12[H2]32

Where,

  • K1 is the equilibrium constant for this reaction.

Simplify the above expression.

K1=[([NH3][N2]12[H2]32)2]12=[[NH3]2[N2][H2]3]12=[K]12

Substitute the given value of K in the above expression.

K1=[K]12=[1.3×102]12=0.11_

Conclusion

The equilibrium constant for the given reaction is 0.11_ .

(b)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The equilibrium constant (K) for each of the given gas-phase reactions is to be stated.

Concept introduction: The state when the reactants involved in a chemical reaction and the products formed in the reaction exist in concentrations having no further tendency to change is known as an equilibrium state of the reaction. When the equilibrium constant is expressed in terms of concentration, it is represented K .

To determine: The equilibrium constant for the given reaction.

Answer to Problem 27E

Answer

The equilibrium constant for the given reaction is 77_ .

Explanation of Solution

Given

The stated reaction is,

2NH3(g)N2(g)+3H2(g)

At equilibrium, the equilibrium constant expression is stated,

K2=[N2][H2]3[NH3]2

Where,

  • K2 is the equilibrium constant for this reaction.

Simplify the above expression.

K2=[[N2][H2]3[NH3]2]=[1K]

Substitute the given value of K in the above expression.

K2=[1K]=[11.3×102]=77_

Conclusion

The equilibrium constant for the given reaction is 77_ .

(c)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The equilibrium constant (K) for each of the given gas-phase reactions is to be stated.

Concept introduction: The state when the reactants involved in a chemical reaction and the products formed in the reaction exist in concentrations having no further tendency to change is known as an equilibrium state of the reaction. When the equilibrium constant is expressed in terms of concentration, it is represented K .

To determine: The equilibrium constant for the given reaction.

Answer to Problem 27E

Answer

The equilibrium constant for the given reaction is 8.8_ .

Explanation of Solution

Given

The stated reaction is,

2NH3(g)12N2(g)+32H2(g)

At equilibrium, the equilibrium constant expression is stated,

K3=[N2]12[H2]32[NH3]

Where,

  • K3 is the equilibrium constant for this reaction.

Simplify the above expression.

K3=[([N2]12[H2]32[NH3])2]12=[[N2][H2]3[NH3]2]12=[1K]12

Substitute the given value of K in the above expression.

K3=[1K]12=[11.3×102]12=8.8_

Conclusion

The equilibrium constant for the given reaction is 8.8_ .

(d)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The equilibrium constant (K) for each of the given gas-phase reactions is to be stated.

Concept introduction: The state when the reactants involved in a chemical reaction and the products formed in the reaction exist in concentrations having no further tendency to change is known as an equilibrium state of the reaction. When the equilibrium constant is expressed in terms of concentration, it is represented K .

To determine: The equilibrium constant for the given reaction.

Answer to Problem 27E

Answer

The equilibrium constant for the given reaction is 1.7×10-4_ .

Explanation of Solution

Given

The stated reaction is,

2N2(g)+6H2(g)4NH3(g)

At equilibrium, the equilibrium constant expression is stated,

K4=[NH3]4[N2]2[H2]6=[[NH3]2[N2][H2]3]2=[K]2

Where,

  • K4 is the equilibrium constant for this reaction.

Substitute the given value of K in the above expression.

K4=[K]2=[1.3×102]2=1.7×10-4_

Conclusion

The equilibrium constant for the given reaction is 1.7×10-4_

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Chapter 13 Solutions

Chemistry

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