Question

state and explan Raout's law​

Answer 1

Answer:

Raoult's law (/ˈrɑːuːlz/ law) is a law of physical chemistry, with implications in thermodynamics. Established by French chemist François-Marie Raoult in 1887,[1] 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. In consequence, the relative lowering of vapour pressure of a dilute solution of nonvolatile solute is equal to the mole fraction of solute in the solution.

Mathematically, Raoult's law for a single component in an ideal solution is stated as

{\displaystyle p_{i}=p_{i}^{\star }x_{i},}{\displaystyle p_{i}=p_{i}^{\star }x_{i},}

where {\displaystyle p_{i}}p_{i} is the partial pressure of the component {\displaystyle i}i in the gaseous mixture (above the solution), {\displaystyle p_{i}^{\star }}{\displaystyle p_{i}^{\star }} is the equilibrium vapor pressure of the pure component {\displaystyle i}i, and {\displaystyle x_{i}}x_{i} is the mole fraction of the component {\displaystyle i}i in the mixture (in the solution).

Explanation:

Answer 2

Answer:

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