ANS:C - Raoult's law

Raoult's Law is a principle in physical chemistry that describes the behavior of ideal solutions. Specifically, it relates to the vapor pressure of a solution consisting of two or more volatile components. The law states that the partial vapor pressure of each component in an ideal solution is directly proportional to its mole fraction in the solution and the vapor pressure of the pure component. In other words, if you have a solution containing two or more substances, each substance will exert a partial pressure in the vapor phase that is proportional to its fraction in the solution. Mathematically, Raoult's Law can be expressed as: 𝑃𝑖=𝑥𝑖⋅𝑃𝑖∗Pi​=xi​⋅Pi∗​ Where:

• 𝑃𝑖Pi​ is the partial vapor pressure of component 𝑖i,
• 𝑥𝑖xi​ is the mole fraction of component 𝑖i in the solution,
• 𝑃𝑖∗Pi∗​ is the vapor pressure of the pure component 𝑖i.

This law holds true only for ideal solutions, where there are no intermolecular interactions between the components of the solution. In real solutions, deviations from Raoult's Law can occur due to factors such as intermolecular forces, molecular size, and non-ideal behavior of the components. When deviations occur, the solution is referred to as non-ideal.