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Questions and Answers
How is the mole fraction calculated?
Why is mole fraction considered dimensionless?
What does the mole fraction represent?
If a mixture contains 2 moles of one substance and 3 moles of another, what is the total mole fraction?
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In a mixture, if a substance has a mole fraction of 0.4, what does this imply?
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In a mixture of hydrogen and oxygen gases with total pressure 104 kPa, what is the partial pressure of oxygen gas?
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What is the total mole fraction in a binary solution if the mole fraction of the solute is 0.4?
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Which scientific discipline typically prefers using mole fraction over concentration when dealing with gas volumes?
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If the mole fraction of a solute in a solution is 0.3, what is the mole fraction of the solvent?
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What happens to the sum of mole fractions in a mixture according to a key relationship?
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Which field is more likely to use molar concentrations like molarity and molality over mole fraction?
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Study Notes
Calculating Mole Fraction
Mole fraction ((X)) is a fundamental concept in chemistry that represents the ratio of the moles of a specific substance to the total moles of all substances present in a mixture. It provides a dimensionless measure of the concentration within a solution. To calculate the mole fraction of a substance, follow these steps:
- Determine the number of moles of the substance you want to find the mole fraction for (let's call this (n_i)).
- Obtain the total number of moles in the entire mixture ((n_{\text{total}})).
- Divide the moles of the substance by the total moles to get the mole fraction: [X_i = \frac{n_i}{n_{\text{total}}}]
Since the mole fraction is dimensionless, it doesn't need any units.
Let's consider an example: A mixture contains 0.5 moles of hydrogen gas (Hâ‚‚) and 1.0 moles of oxygen gas (Oâ‚‚). Assuming the total pressure is 104 kPa, how do we find the partial pressure of each gas?
First, let's determine the mole fractions: [ X_{\text{H}2} = \frac{0.5 :\text{mol}}{0.5 :\text{mol} + 1.0 :\text{mol}} = 0.33 ] [ X{\text{O}2} = \frac{1.0 :\text{mol}}{0.5 :\text{mol} + 1.0 :\text{mol}} = 0.67 ] Now, considering the total pressure is 104 kPa, we can find the partial pressures using their respective mole fractions: [ P{\text{H}2} = X{\text{H}2} \cdot P{\text{total}} = 0.33 \cdot 104 :\text{kPa} = 34.6 :\text{kPa} ] [ P_{\text{O}2} = X{\text{O}2} \cdot P{\text{total}} = 0.67 \cdot 104 :\text{kPa} = 69.2 :\text{kPa} ] So, the partial pressure of hydrogen gas is approximately 34.6 kPa, while that of oxygen gas is around 69.2 kPa.
It's worth mentioning that the sum of all mole fractions in a mixture adds up to 1: [ \sum_{i=1}^n X_i = 1 ] This relationship ensures consistency within the molecular proportions present in the mixture.
Mole Fraction in Solutions
In the context of solutions, the mole fraction becomes particularly important because it helps describe the distribution of solutes and solvents. For binary solutions, the mole fraction of the solvent is simply the inverse of the mole fraction of the solute: [ X_{\text{solvent}} + X_{\text{solute}} = 1 ] If you know the mole fraction of either the solvent or the solute, you can easily obtain the other.
Relationship Between Mole Fraction and Concentration
While mole fraction and concentration are related concepts, there exists some confusion due to the variety of definitions and terminologies used across scientific disciplines. In physical chemistry, mole fraction is preferred over concentration, especially in dealing with gas volumes. On the other hand, molar concentrations, such as molarity and molality, are more commonly used in fields like biochemistry and pharmacology.
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Description
Learn how to calculate mole fractions of substances in mixtures and solutions. Understand the relationship between mole fractions, partial pressures, and concentrations. Practice determining mole fractions in a variety of scenarios.
