   # Nitrogen and oxygen can react to form nitrogen monoxide according to the following chemical equation N 2 ( g ) + O 2 ( g ) ⇄ 2 N O ( g ) (a) Calculate Δ r G ° for this reaction at 298 K using values for the standard free energies of formation of the product and reactants. Is this reaction reactant-favored or product-favored at equilibrium? (b) Calculate the value of Δ r G at 298 K for this reaction if the reactants and product are mixed with the following partial pressures: 0.10 atm N 2 , 0.10 atm O 2 , and 0.010 atm NO. Is this reaction spontaneous under these conditions? ### Chemistry & Chemical Reactivity

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

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 18.7, Problem 6CYU
Textbook Problem
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## Nitrogen and oxygen can react to form nitrogen monoxide according to the following chemical equation N 2 ( g ) + O 2 ( g ) ⇄ 2   N O ( g ) (a) Calculate ΔrG° for this reaction at 298 K using values for the standard free energies of formation of the product and reactants. Is this reaction reactant-favored or product-favored at equilibrium? (b) Calculate the value of ΔrG at 298 K for this reaction if the reactants and product are mixed with the following partial pressures: 0.10 atm N2, 0.10 atm O2, and 0.010 atm NO. Is this reaction spontaneous under these conditions?

(a)

Interpretation Introduction

Interpretation:

The ΔrG° for the given reaction N2(g)+O2(g)2NO(g) should be calculated using standard free energies of reactant and product formation and should be identified that whether reaction is reactant or product favoured.

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)

ΔrGo gets related to the reaction quotient Q by the expression ΔrG = ΔrG°+ RT lnQ

For a general reaction, aA + bBcC + dD

Q = [C]c[D]d[A]a[B]b

### Explanation of Solution

The ΔrG° for the given reaction is calculated below.

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

The Appendix L was referred for the values of standard free energy.

The ΔrG° for NO(g) is 86.58 kJ/mol

The ΔrG° for N2(g) is 0 kJ/mol

The ΔrG° for O2(g) is 0 kJ/mol

ΔrG°fG°(products)fG°(reactants)

ΔrG°[(2 mol NO(g)/mol-rxn)ΔfG°[

(b)

Interpretation Introduction

Interpretation:

The ΔrG° for the reaction when 0.10 atmN2,0.10atm O2and0.010atm NO are mixed should be calculated and should be identified that whether this reaction is spontaneous or not under such given conditions.

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)

ΔrGo gets related to the reaction quotient Q by the expression ΔrG = ΔrG°+ RT lnQ

For a general reaction, aA + bBcC + dD

Q = [C]c[D]d[A]a[B]b

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