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Expressing Concentration of Solution: Mole Fraction Video Lecture | Chemistry for JEE Main & Advanced
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FAQs on Expressing Concentration of Solution: Mole Fraction Video Lecture - Chemistry for JEE Main & Advanced
| 1. What is mole fraction and how is it calculated? |  |
Ans. Mole fraction is a way to express the concentration of a component in a solution. It is calculated by dividing the moles of the component by the total moles of all components in the solution.
| 2. How is mole fraction different from molarity? | |
Ans. Mole fraction is a dimensionless quantity that represents the ratio of moles of a component to the total moles in a solution, while molarity is a measure of the concentration of a solute in a solution, expressed as the number of moles of solute per liter of solution.
| 3. Can the mole fraction of a component exceed 1? | |
Ans. No, the mole fraction of a component cannot exceed 1. Mole fraction is a ratio and is always expressed as a decimal value between 0 and 1, inclusive.
| 4. How is mole fraction useful in determining vapor pressure? | |
Ans. Mole fraction is useful in determining the vapor pressure of a solution through Raoult's law. According to Raoult's law, the vapor pressure of a component in a solution is directly proportional to its mole fraction in the solution.
| 5. Is mole fraction affected by changes in temperature and pressure? | |
Ans. No, mole fraction is independent of changes in temperature and pressure. It is a ratio of moles and does not change with variations in external conditions. However, the mole fraction of a component can change if the composition of the solution is altered by adding or removing other components.
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