   Chapter 15, Problem 63GQ

Chapter
Section
Textbook Problem

A sample of N2O4 gas with a pressure of 1.00 atm is placed in a flask. When equilibrium is achieved, 20.0% of the N2O4 has been convened to NO2 gas. (a) Calculate Kp. If the original pressure of N2O4 is 0.10 atm, what is the percent dissociation of the gas? Is the result in agreement with Le Chatelier’s principle?

(a)

Interpretation Introduction

Interpretation:

The KP for the dissociation reaction of N2O4 to NO2 with a pressure of 1atm has to be calculated.

Concept Introduction:

• Partial pressure: The pressure of each gas in a mixture of gases is the partial pressure.
• Dalton’s law of partial pressure: The total pressure of gases in a mixture of gases is the sum of the pressure of each gas in the mixture
• Mole fraction: Quantity which defines the number of moles of a substance in a mixture divided by the total number of moles of all substances present.

xa=nantotal

• pa=xa×Ptotal

Partial pressure of a gas in the mixture of gases is the product of mole fraction of the gas and the total pressure.

• Ideal gas equation:PV=nRT

Equilibrium constant in terms of pressure[Kp]: Equilibrium constant can be expressed in terms of partial pressures in atmospheres.

• aA(g)+bB(g)cC(g)+dD(g)KP=PCc×PDdPAa×PBb

Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Explanation

Given:

N2O42NO2Pressure=1atmAtequilibrium,20%N2O4convertstoNO2

Given that initial pressure is 1atm

Given the reaction:

N2O42NO2Initialpressure1atm0Change

(b)

Interpretation Introduction

Interpretation:

The percent of dissociation of gas if the original pressure of N2O4 is 0.10atm has to be given.

Concept Introduction:

• Partial pressure: The pressure of each gas in a mixture of gases is the partial pressure.
• Dalton’s law of partial pressure: The total pressure of gases in a mixture of gases is the sum of the pressure of each gas in the mixture
• Mole fraction: Quantity which defines the number of moles of a substance in a mixture divided by the total number of moles of all substances present.

xa=nantotal

• pa=xa×Ptotal

Partial pressure of a gas in the mixture of gases is the product of mole fraction of the gas and the total pressure.

• Ideal gas equation:PV=nRT

Equilibrium constant in terms of pressure[Kp]: Equilibrium constant can be expressed in terms of partial pressures in atmospheres.

• aA(g)+bB(g)cC(g)+dD(g)KP=PCc×PDdPAa×PBb

Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

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