Raoult's Law and Its Applications
Chemistry ⇒ Solutions and Colloids
Raoult's Law and Its Applications starts at 11 and continues till grade 12.
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A binary solution of A and B has xA = 0.4, PA0 = 100 mmHg, and PB0 = 60 mmHg. Calculate the total vapor pressure of the solution.
A binary solution of liquids A and B has mole fractions xA = 0.3 and xB = 0.7. The vapor pressures of pure A and B are 120 mmHg and 80 mmHg, respectively. Calculate the partial vapor pressure of B.
A solution contains 0.1 mol of non-volatile solute and 0.9 mol of solvent. If the vapor pressure of pure solvent is 40 mmHg, what is the vapor pressure of the solution?
A solution contains 0.2 mol of solute and 0.8 mol of solvent. If the vapor pressure of pure solvent is 50 mmHg, what is the vapor pressure of the solution?
A solution contains 0.3 mol of solute and 0.7 mol of solvent. If the vapor pressure of pure solvent is 60 mmHg, what is the relative lowering of vapor pressure?
A solution is made by dissolving 10 g of a non-volatile solute in 90 g of water. The vapor pressure of pure water at 25°C is 23.8 mmHg. If the mole fraction of water is 0.95, what is the vapor pressure of the solution?
A solution is prepared by dissolving 5 g of a non-volatile solute in 95 g of water. The vapor pressure of pure water is 23.8 mmHg. The vapor pressure of the solution is 23.0 mmHg. Calculate the mole fraction of the solute.
A solution is prepared by mixing 0.5 mol of ethanol and 0.5 mol of methanol. The vapor pressures of pure ethanol and methanol at 25°C are 44 mmHg and 88 mmHg, respectively. Calculate the total vapor pressure of the solution assuming ideal behavior.
A solution of urea (non-volatile) in water has a vapor pressure of 23.5 mmHg at 25°C. The vapor pressure of pure water at this temperature is 25 mmHg. Calculate the mole fraction of water in the solution.
Describe how Raoult's Law is used to determine the molar mass of a non-volatile solute.
Describe the effect of adding a non-volatile solute to a solvent on its vapor pressure.
Describe the main difference between ideal and non-ideal solutions with respect to Raoult's Law.
Describe the relationship between Raoult's Law and Dalton's Law of Partial Pressures.
Explain the significance of azeotropes in the context of Raoult's Law.
Explain the term 'partial vapor pressure' in the context of Raoult's Law.
Explain why Raoult's Law fails for solutions with strong solute-solvent interactions.
Explain why solutions showing positive deviation from Raoult's Law have higher vapor pressure than predicted.
Explain why the vapor pressure of a solution is not simply the average of the vapor pressures of the pure components.
State Raoult's Law for an ideal solution.
The vapor pressure of pure solvent A at 25°C is 100 mmHg. If the mole fraction of A in a solution is 0.8, what is the partial vapor pressure of A according to Raoult's Law?
