Equal weight of a solute are dissolved in equal weight of two solvents \(A\) and \(B\) and formed very dilute solution. The relative lowering of vapour pressure for the solution \(B\) has twice the relative lowering of vapour pressure for the solution \(A\). If \(M_{A}\) and \(M_{B}\) are the molecular weights of solvents \(A\) and \(B\) respectively, then: (a) \(M_{A}=M_{B}\) (b) \(M_{B}=2 \times M_{A}\) (c) \(M_{A}=4 M_{B}\) (d) \(M_{A}=2 M_{B}\)

Raoult's law is a fundamental principle in chemistry that describes how the vapor pressure of a solution is related to the concentration of solute particles in the solution. Simply put, it states that the vapor pressure of an ideal solution is directly proportional to the mole fraction of the solvent. This relationship can be mathematically expressed as:
\( P = P^0_{solvent} \times X_{solvent} \),
where \( P \) is the vapor pressure of the solution, \( P^0_{solvent} \) is the vapor pressure of the pure solvent, and \( X_{solvent} \) is the mole fraction of the solvent in the solution. Understanding Raoult's law is essential for solving problems related to the vapor pressure of solutions, including the determination of molar masses and calculation of mole fractions.

Determining the molar mass is vital for interpreting many aspects of chemical behavior, and it can be done by measuring changes in physical properties, such as vapor pressure. In the provided exercise, we see how the relative lowering of vapor pressure assists in determining the molar mass of the solvents. By analyzing the ratio of the vapor pressure reduction, we indirectly compare molar masses. The use of the formula:
\( n_{solvent} = \frac{w_{solvent}}{M_{solvent}} \)
allows us to calculate the number of moles based on the known weight and the unknown molar mass. When the weight of solute and solvent is constant, as in our exercise, the relative lowering of vapor pressure can be a direct indicator of the molar mass ratio between two solvents.

The mole fraction is a dimensionless quantity that represents the ratio of the number of moles of a component to the total number of moles of all components in the solution. It is an essential concept when discussing mixtures and solutions in chemistry. For a two-component system such as a solute dissolved in a solvent, the mole fraction of each component is defined as:
\( X_i = \frac{n_i}{n_{total}} \)
where \( X_i \) is the mole fraction of component \( i \) and \( n_i \) and \( n_{total} \) are the number of moles of component \( i \) and the total number of moles, respectively. In the context of the exercise, Raoult's law connects mole fraction to vapor pressure, illustrating that the mole fraction is a crucial parameter in determining physical properties of solutions such as boiling point, freezing point, and vapor pressure.