Question

1) Define Raoult's law for liquid in liquid solutions
2) What is meant by positive deviation from Raoult's law?
3) Give an example for negative deviation from Raoult's law?
4) Why more vapoure pressure in case of positive deviation from Raoult's law?
5) Define azeotrope mixture?​

Answer 1

Answer:

1. Established by French chemist François-Marie Raoult in 1887, it states that the partial pressure of each component of an ideal mixture of liquids is equal to the vapour pressure of the pure component multiplied by its mole fraction in the mixture.
2. Deviations from Raoult's law can either be positive or negative. A positive deviation means that there is a higher than expected vapor pressure above the solution. A negative deviation, conversely, means that we find a lower than expected vapor pressure for the solution.
3. Negative deviation from raoult's law means that the total vapour pressure of the initial liquid will be more when compared to the total vapour pressure of the solution ( when both the liquids are mixed ). eg. solution of Nitric and Water.
4. When the cohesive forces between like molecules are greater than the adhesive forces between dissimilar molecules, the dissimilarities of polarity leads both components to escape solution more easily. Therefore, the vapor pressure is greater than expected from the Raoult's law, showing positive deviation.

5. Azeotrope, in chemistry, a mixture of liquids that has a constant boiling point because the vapour has the same composition as the liquid mixture. The boiling point of an azeotropic mixture may be higher or lower than that of any of its components.

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