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What does point A signify in the figure given below?
What does point A signify in the figure given below?
One component of a solution follows Raoult's law over the entire range $0 ≤ x_1 ≤ 1$. The second component must follow Raoult's law in the range when $x_2$ is
One component of a solution follows Raoult's law over the entire range $0 ≤ x_1 ≤ 1$. The second component must follow Raoult's law in the range when $x_2$ is
If two substances A and B have $p°_A : p°_B = 1:2$ and the mole fraction in solution = 1:2 then the mole fraction of A in vapours is
If two substances A and B have $p°_A : p°_B = 1:2$ and the mole fraction in solution = 1:2 then the mole fraction of A in vapours is
At 300 K, two pure liquids A and B have 150 mm Hg and 100 mm Hg vapour pressures, respectively. In an equimolar liquid mixture of A and B, the mole fraction of B in the vapour mixture at this temperature is
At 300 K, two pure liquids A and B have 150 mm Hg and 100 mm Hg vapour pressures, respectively. In an equimolar liquid mixture of A and B, the mole fraction of B in the vapour mixture at this temperature is
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Vapour pressure of chloroform ($CHCl_3$) and dichloromethane ($CH_2Cl_2$) at 25°C are 200 mm of Hg and 41.5 mm of Hg respectively. Vapour pressure of the solution obtained by mixing 25.5 g of $CHCl_3$ and 40 g of $CH_2Cl_2$ at the same temperature will be
Vapour pressure of chloroform ($CHCl_3$) and dichloromethane ($CH_2Cl_2$) at 25°C are 200 mm of Hg and 41.5 mm of Hg respectively. Vapour pressure of the solution obtained by mixing 25.5 g of $CHCl_3$ and 40 g of $CH_2Cl_2$ at the same temperature will be
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When does Raoult's law become a special case of Henry's law?
When does Raoult's law become a special case of Henry's law?
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Study Notes
Solution Properties and Laws
- Point A in a pressure vs. mole fraction figure signifies the vapor pressure of the pure solvent.
- Raoult's law applies to one component of a solution across the entire mole fraction range, indicating that the second component may only follow Raoult's law when its mole fraction is close to zero.
- In a mixture of two components A and B, the vapor phase mole fraction of A can be calculated from their vapor pressures and mole fractions in solution, yielding specific values based on ratios.
Vapor Pressure Calculations
- Equimolar mixtures result in specific mole fractions in vapor; for example, at 300 K, the mole fraction of component B in the vapor mixture from liquids A (150 mm Hg) and B (100 mm Hg) yields a mole fraction of B close to 0.6.
- When mixing chloroform (200 mm Hg) and dichloromethane (41.5 mm Hg), molecular masses are crucial for calculating the resultant vapor pressure of their mixture. Based on a specific combination of 25.5 g of chloroform and 40 g of dichloromethane, the vapor pressure would be calculated to be 173.9 mm Hg.
Special Cases of Laws
- Raoult's law can be seen as a particular instance of Henry's law under specific conditions, emphasizing its broader application in physical chemistry.
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Description
Test your understanding of solutions with this quiz focused on key concepts like vapor pressure and Raoult's law. Each question will challenge your grasp of how solutes and solvents interact in chemical solutions. Perfect for chemistry students looking to reinforce their knowledge!
