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The Haber-Bosch process for the production of ammonia is one of the key industrial processes in developed countries. N 2 ( g ) + 3H 2 ( g ) ⇄ 2NH 3 ( g ) (a) Calculate Δ r G ° for the reaction at 298 K, 800 K, and 1300 K. Data at 298 K are given in Appendix L Data for the other temperatures are as follows: How does the Δ r G ° change with temperature? (b) Calculate the equilibrium constant for the reaction at 298 K, 800 K, and 1300 K. (c) At what temperature (298 K, 800 K, or 1300 K) is the mole fraction of NH 3 the greatest?

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Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

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Chapter
Section
BuyFindarrow_forward

Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 18, Problem 87SCQ
Textbook Problem
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The Haber-Bosch process for the production of ammonia is one of the key industrial processes in developed countries.

N2(g) + 3H2(g) ⇄ 2NH3(g)

(a) Calculate ΔrG° for the reaction at 298 K, 800 K, and 1300 K. Data at 298 K are given in Appendix L Data for the other temperatures are as follows:

Chapter 18, Problem 87SCQ, The Haber-Bosch process for the production of ammonia is one of the key industrial processes in

How does the ΔrG° change with temperature?

(b) Calculate the equilibrium constant for the reaction at 298 K, 800 K, and 1300 K.

(c) At what temperature (298 K, 800 K, or 1300 K) is the mole fraction of NH3 the greatest?

(a)

Interpretation Introduction

Interpretation:

The free energy change values for given temperatures and the response of it with respect to the temperature should be identified.

Concept introduction:

The Gibbs free energy or the free energy change is a thermodynamic quantity represented by ΔrG. It can be calculated in a similar manner as entropy and enthalpy.  The expression for the free energy change is:

  ΔrG°fG°(products)fG°(reactants)

ΔGo is related to the equilibrium constant K by the equation,

  ΔrGo= -RTlnKp

The rearranged expression is,

  Kp=e-ΔrGoRT

It is also related to entropy and entropy by the following expression,

  ΔGo= ΔHo-TΔSo

Here, ΔHo is the change in enthalpy and ΔSo is the change in entropy.

Explanation of Solution

The ΔrGo for the given reaction at different temperature is calculated below.

Given:

Refer to Appendix L for the values of standard free energy, standard entropy and standard enthalpy values.

The given reaction is,

  N2(g)+3H2(g)2NH3(g)

At 298 K,

The ΔfG° for NH3(g) is 16.37 kJ/mol.

The ΔfG° for H2(g) is 19.33 kJ/mol.

The ΔfG° for N2(g) is 0 kJ/mol.

  ΔrG°fG°(products)fG°(reactants)=[(2 mol NH3(g)/mol-rxn)ΔfG°[NH3(g)]-[(3 mol H2(g)/mol-rxn)ΔfG°[H2(g)]+(1 mol N2(g)/mol-rxn)ΔfG°[N2(g)]]] 

Substitute the values,

  ΔrG°=[(2 mol NH3(g)/mol-rxn)(-16

(b)

Interpretation Introduction

Interpretation:

The equilibrium constant values for given temperatures should be identified.

Concept introduction:

The Gibbs free energy or the free energy change is a thermodynamic quantity represented by ΔrG. It can be calculated in a similar manner as entropy and enthalpy.  The expression for the free energy change is:

  ΔrG°fG°(products)fG°(reactants)

ΔGo is related to the equilibrium constant K by the equation,

  ΔrGo= -RTlnKp

The rearranged expression is,

  Kp=e-ΔrGoRT

It is also related to entropy and entropy by the following expression,

  ΔGo= ΔHo-TΔSo

Here, ΔHo is the change in enthalpy and ΔSo is the change in entropy.

(c)

Interpretation Introduction

Interpretation:

The temperature at which mole fraction of given species will be greatest should be identified. 

Concept introduction:

The Gibbs free energy or the free energy change is a thermodynamic quantity represented by ΔrGo. It can be calculated in a similar manner as entropy and enthalpy.  The expression for the free energy change is:

  ΔrG°fG°(products)fG°(reactants)

ΔGo is related to the equilibrium constant K by the equation,

  ΔrGo= -RTlnKp

The rearranged expression is,

  Kp=e-ΔrGoRT

It is also related to entropy and entropy by the following expression,

  ΔGo= ΔHo-TΔSo

Here, ΔHo is the change in enthalpy and ΔSo is the change in entropy.

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Chapter 18 Solutions

Chemistry & Chemical Reactivity
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