   Chapter 13, Problem 112CP

Chapter
Section
Textbook Problem

# A sample of N2O4(g) is placed in an empty cylinder at 25°c. After equilibrium is reached the total pressure is 1.5 atm and 16% (by moles) of the original N2O4(g) has dissociated to NO2(g).a. Calculate the value of Kp for this dissociation reaction at 25°C.b. If the volume of the cylinder is increased until the total pressure is 1.0 atm (the temperature of the system remains constant), calculate the equilibrium pressure of N2O 4(g) and NO2 (g).c. What percentage (by moles) of the original N2O4(g) is dissociated at the new equilibrium position (total pressure = l.00 atm)?

(a)

Interpretation Introduction

Interpretation: The equilibrium constant Kp for the dissociation reaction has to be calculated.

Concept introduction: The equilibrium constant Kp describes the ratio of the reactant to the product on the equilibrium conditions in terms of the partial pressure.

At equilibrium sum of all the partial pressure is equal to the total pressure.

Law of mass action is applicable on the equilibrium reactions.

Dissociation is also known as degree of dissociation which tells that dissociated amount of the species at a particular time.

To determine: The equilibrium constant Kp for the dissociation reaction.

Explanation

Explanation

The equilibrium constant Kp for the dissociation reaction is 0.16atm_

Given

The reaction is given as,

N2O4(g)2NO2(g)

At equilibrium the total pressure Ptotal=1.5atm at 25°C .

The percent dissociation of N2O4=16%

The initial pressure of N2O4 is assumed to be x . The ICE-chart that is the initial pressure, change in pressure and equilibrium pressure is given as,

N2O4(g)2NO2(g)Initialpressurex0Changeinpressure(0.16)x+(0.32)xEquilibriumpressure(0.84)x(0.32)x

At equilibrium the partial pressure is equal to the sum of the individual pressure of the all gases. Therefore,

Ptotal=Ppartial

Where,

• Ptotal is the total pressure at equilibrium.
• Ppartial is the partial pressure of the gases

(b)

Interpretation Introduction

Interpretation: The equilibrium pressure of N2O4(g) and NO2(g) is to be calculated. At the new equilibrium position the mole percentage of the undissociated N2O4 is to be calculated.

Concept introduction: The equilibrium constant Kp describes the ratio of the reactant to the product on the equilibrium conditions in terms of the partial pressure.

At equilibrium sum of all the partial pressure is equal to the total pressure.

Law of mass action is applicable on the equilibrium reactions.

Dissociation is also known as degree of dissociation which tells that dissociated amount of the species at a particular time.

To determine: The equilibrium pressure of N2O4(g) and NO2(g) .

(c)

Interpretation Introduction

Interpretation:At the new equilibrium position the mole percentage of the undissociated N2O4 is to be calculated.

Concept introduction: The equilibrium constant Kp describes the ratio of the reactant to the product on the equilibrium conditions in terms of the partial pressure.

At equilibrium sum of all the partial pressure is equal to the total pressure.

Law of mass action is applicable on the equilibrium reactions.

Dissociation is also known as degree of dissociation which tells that dissociated amount of the species at a particular time.

To determine: The dissociated percentage of original N2O4(g) at new equilibrium position.

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