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# Mole Fraction

## Introduction to calculations used to express relative amounts of substances in a mixture

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Mole Fraction

Credit: Courtesy of J. D. Griggs, US Geological Survey
Source: http://commons.wikimedia.org/wiki/File:Pahoeoe_fountain_sharpen.jpg
License: CC BY-NC 3.0

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### Mole Fraction

One way to express relative amounts of substances in a mixture is with the mole fraction. Mole fraction (X)\begin{align*}(X)\end{align*} is the ratio of moles of one substance in a mixture to the total number of moles of all substances. For a mixture of two substances, A\begin{align*}A\end{align*} and B\begin{align*}B\end{align*}, the mole fractions of each would be written as follows:

XA=mol Amol A+mol BandXB=mol Bmol A+mol B

If a mixture consists of 0.50 mol A\begin{align*}A\end{align*} and 1.00 mol B\begin{align*}B\end{align*}, then the mole fraction of A\begin{align*}A\end{align*} would be XA=0.51.5=0.33\begin{align*}X_A=\frac{0.5}{1.5} = 0.33\end{align*}.  Similarly, the mole fraction of B\begin{align*}B\end{align*} would be XB=1.01.5=0.67\begin{align*}X_B =\frac{1.0}{1.5} = 0.67\end{align*}.

Mole fraction is a useful quantity for analyzing gas mixtures in conjunction with Dalton’s law of partial pressures. Consider the following situation: A 20.0 liter vessel contains 1.0 mol of hydrogen gas at a pressure of 600 mmHg. Another 20.0 liter vessel contains 3.0 mol of helium at a pressure of 1800 mmHg. These two gases are mixed together in an identical 20.0 liter vessel. Because each will exert its own pressure according to Dalton’s law, we can express the partial pressures as follows:

PH2=XH2×PTotalandPHe=XHe×PTotal

The partial pressure of a gas in a mixture is equal to its mole fraction multiplied by the total pressure. For our mixture of hydrogen and helium:

XH2=1.0 mol1.0 mol+3.0 mol=0.25andXHe=3.0 mol1.0 mol+3.0 mol=0.75

The total pressure according to Dalton’s law is 600 mmHg+1800 mmHg=2400 mmHg\begin{align*}600 \text{ mmHg} + 1800 \text{ mmHg} = 2400 \text{ mmHg}\end{align*}. So, each partial pressure will be:

PH2=0.25×2400 mmHg=600 mmHgPHe=0.75×2400 mmHg=1800 mmHg

The partial pressures of each gas in the mixture don’t change since they were mixed into the same size vessel and the temperature was not changed.

#### Sample Problem: Dalton’s Law

A flask contains a mixture of 1.24 moles of hydrogen gas and 2.91 moles of oxygen gas. If the total pressure is 104 kPa, what is the partial pressure of each gas?

Step 1: List the known quantities and plan the problem.

Known

• 1.24 mol H2
• 2.91 mol O2
• PTotal=104 kPa\begin{align*}P_{\text{Total}}=104 \ \text{kPa}\end{align*}

Unknown

• PH2=? kPa\begin{align*}P_{H_2}=? \ \text{kPa}\end{align*}
• PO2=? kPa\begin{align*}P_{O_2}=? \ \text{kPa}\end{align*}

First, the mole fraction of each gas can be determined. Then, the partial pressure can be calculated by multiplying the mole fraction by the total pressure.

Step 2: Solve.

XH2=1.24 mol1.24 mol+2.91 mol=0.299PH2=0.299×104 kPa=31.1 kPaXO2=2.91 mol1.24 mol+2.91 mol=0.701PO2=0.701×104 kPa=72.9 kPa

The hydrogen is slightly less than one third of the mixture, so it exerts slightly less than one third of the total pressure.

#### Summary

• Use of the mole fraction allows calculation to be made for mixtures of gases.

#### Practice

Questions

Watch the video at the link below and answer the following questions:

1. What is mole percent?
2. Do the mole fractions add up to 1.00?
3. What other way could you calculate the mole fraction of oxygen once you have the mole fraction of nitrogen?

#### Review

Questions

1. What is mole fraction?
2. How do you determine partial pressure of a gas when given the mole fraction and the total pressure?
3. In a gas mixture containing equal numbers of moles of two gases, what can you say about the partial pressures of each gas?