The boiling point of `0.2 mol kg^(-1)` solution of `X` in water is greater than equimolal solution of `Y` in water. Which of the following statements is true in this case?

Options

A. Y is undergoing dissociation in water while X indergoes no change
B. X is undergoing dissociation in water
C. Molecular mass of X is greater than the molecular mass of Y
D. Molecular of X is less than the molecular mass of Y.

Answer

2

Explanation

We have
`DeltaT_(b)=iK_(b)m`
For equimolal aqueous solutions, `K_(b)` and m are identical. Thus, `DeltaT_(b)` is directly proportional to the value of van't hoff factor. The higher boiling point of aqueous solution of `X` clearly indicates that. It has higher value of i. In case of dissociation, `igt 1`.