Raoult's Law and Henry's Law Quiz and Flashcards

Study Notes

Henry's Law and Gas Solubility

The solubility of a gas in a liquid is directly proportional to the partial pressure of the gas, as stated by Henry's Law.
The law can be expressed mathematically as: C = k * P, where C is the concentration of the gas in the liquid, k is Henry's Law constant, and P is the partial pressure of the gas.

Ideal Solutions

Ideal solutions are mixtures of two or more components that behave ideally, meaning they follow Raoult's Law and Henry's Law.
One characteristic property of ideal solutions is that the vapor pressure of the solution is directly proportional to the mole fraction of each component.

Osmosis Reversal

The reversal of the osmosis process occurs when the osmotic pressure of the more concentrated solution is greater than the external pressure applied to the system.

Raoult's Law and Vapor Pressure

Raoult's Law states that the vapor pressure of a solution is proportional to the mole fraction of the solvent.
The law can be expressed mathematically as: P = P° * x, where P is the vapor pressure of the solution, P° is the vapor pressure of the pure solvent, and x is the mole fraction of the solvent.

Relative Lowering of Vapor Pressure

The relative lowering of vapor pressure is defined as the ratio of the vapor pressure of the solution to the vapor pressure of the pure solvent.
Mathematically, it can be expressed as: ΔP/P° = (P° - P) / P°.

Multiple Non-Volatile Solutes

In a solution with multiple non-volatile solutes, the equation for the reduction in vapor pressure simplifies to: P = P° * x, where x is the mole fraction of the solvent.

Positive Deviation from Raoult's Law

Positive deviation from Raoult's Law occurs when the intermolecular forces between the solute and solvent molecules are weaker than the forces between the solvent molecules.
Positive deviation causes the vapor pressure of the solution to be greater than predicted by Raoult's Law.
Mixtures of ethanol and acetone show positive deviation from Raoult's Law due to the weak hydrogen bonding between the molecules.
Positive deviation is caused by the presence of weak intermolecular forces, such as London dispersion forces or weak hydrogen bonding, between the solute and solvent molecules.

Description

Test your knowledge on the principles of Henry’s Law and Raoult’s Law, which govern the dissolution of gases in liquids and the lowering of vapor pressure in solutions. Understand the relationships between gas solubility, partial pressure, and solute concentration in solutions.