   Chapter 10, Problem 38PS

Chapter
Section
Textbook Problem

A cylinder of compressed gas is labeled “Composition (mole %): 4.5% H2S, 3.0% CO2, balance N2.” The pressure gauge attached to the cylinder reads 46 atm. Calculate the partial pressure of each gas, in atmospheres, in the cylinder.

Interpretation Introduction

Interpretation:

The partial pressure of each gas in the cylinder has to be given.  The composition is given as 4.5%H2S,3%CO2,92.5%N2

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

• Mole percent: It can be calculated by simply multiplying mole fraction by 100.

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.

Explanation

Given the mole percentage of the gases in the mixture:

H2S-4.5%CO2-3%N2-92.5%

From mole percent we can easily calculate the mole fraction of the compound. If we multiply mole fraction by 100 we get the mole percent. So mole fraction can be determined by dividing mole percent by 100.

MolefractionofH2S,xH2S=4.5/100=0.045MolefractionofCO2,xCO2=3/100=0.03MolefractionofN2,xN2=92.5/100=0

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