## What is Raoult’s Law Class 12?

Raoult’s Law for Volatile Solutes Raoult’s law states that in a solution, the vapour pressure of a component at a given temperature is equal to the mole fraction of that component in the solution multiplied by the vapour pressure of that component in the pure state.

## What is Raoult’s Law of lowering of Vapour pressure?

Raoult’s law states that the relative lowering in vapour pressure of a solution containing a nonvolatile solute is equal to the mole fraction of solute in the solution.

## How do you calculate the vapor pressure of a solution?

The vapour pressure of a solution of a non-volatile solute is equal to the vapour pressure of the pure solvent at that temperature multiplied by its mole fraction. In equation form, this reads: In this equation, Po is the vapour pressure of the pure solvent at a particular temperature.

## What is Raoult’s Law and its application?

One of the simplest and most widely applied for non- aqueous mixtures is Raoult’s law. It is used to estimate the contribution of individual components of a liquid or solid mixture to the total pressure exerted by the system, espe- cially for discrete mixtures where the quantity of each com- ponent is known.

## What is P in Raoult’s Law?

Raoult’s law is a chemical law that states that the vapor pressure of a solution is dependent on the mole fraction of a solute added to the solution. Raoult’s Law is expressed by the formula: Psolution = ΧsolventPsolvent.

## What is Raoult’s Law and Henry’s law?

Raoult’s law describes the dependence of the vapour pressure of a solvent as a function of its mole fraction χ1: limχ1→1(pχ1)=p∗ where p∗ is the vapour pressure of the pure solvent. Henry’s law describes the dependence of the vapour pressure of a solute as a function of its concentration.

## In which case Raoult’s Law is not applicable?

Raoult’s law is applicable only to very dilute solutions. Raoult’s law is applicable to solutions containing non-volatile solute only. Raoult’s law is not applicable to solutes which dissociate or associate in the particular solution.

## What are the 4 Colligative properties?

These colligative properties include vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure. This small set of properties is of central importance to many natural phenomena and technological applications, as will be described in this module.

## How do you calculate Molality?

A final way to express the concentration of a solution is by its molality. The molality ( m ) of a solution is the moles of solute divided by the kilograms of solvent. A solution that contains 1.0 mol of NaCl dissolved into 1.0 kg of water is a “one-molal” solution of sodium chloride.

## What is the equation for osmotic pressure?

The equation for osmotic pressure is pi=iMRT. The higher the concentration (M) or the temperature (T) of a solution, the higher the osmotic pressure.

## Is NaCl volatile?

Sodium chloride (NaCl; table salt) is not volatile. It has a boiling point of 1413oC and does not evaporate readily even at elevated temperatures. It is not flammable or explosive.

## What is Henry’s Law equation?

L. mol1 and C = 2*105 M into the Henry’s law formula: P = kH*C = (1.6*103 atm. L.

## What is ideal and non ideal solutions?

The solution which obey Raoult’s law over the entire range of concentration are known as ideal solutions. When a solution does not obey Raoults’s law it is called as non-ideal solution.

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