Limitations of Henry's Law and Raoult's Laws

Henry's Law :

This law is applicable when the solute is a gas while the solvent is a liquid i.e. in a gas-liquid solution. It states that, “The pressure of a gas above a gas-liquid solution is directly proportional to its mole fraction in the solution”.

Limitations of Henry's Law :

This law is applicable only when:

• The gas does not undergo any chemical change.
• The gas does not undergo association or dissociation in the solution.
• The pressure of the gas is not too high and temperature is not too low.

Rauolt's law:

This law is generally considered in liquid-liquid solutions. It states that,”The partial vapour pressure of liquid component of an ideal solution is directly proportional to its mole fraction in the solution”.

Limitations of Rauolt's law:

• Raoult's law is not applicable to solutes which either dissociate or associate when dissolved in the particular solvent i.e. this law is applicable to solutions containing non-volatile and non-electrolyte solutes.
• This law is applicable only to very dilute solutions.
• Inter-molecular forces of attraction between the two liquid components in the solution should be similar to those inter-molecular forces of attraction between individual molecules i.e. if we have a solution of A and B liquids, then the inter-molecular forces of attraction between A-A = B-B = A-B

i.e. this law is not applicable to non-ideal solutions.

Also see:

EXCEPTIONS AND AMAZING FACTS ABOUT CHEMISTRY

• Tweet
• Share
• Share
• Share
• Share

About Admin MC3

This is dummy text. It is not meant to be read. Accordingly, it is difficult to figure out when to end it. But then, this is dummy text. It is not meant to be read. Period.

Related Post