The ideal solutions formed by mixing two liquids $A$ and $B$ at $300 \ K$ in the molar ratio of $1:1$ and $1:2$ have vapour pressures of $400 \ mm$ and $350 \ mm$ respectively. At the same temperature,the vapour pressures of pure liquids $A$ and $B$ in $mm$ respectively are:

Identify the false statement among the following.

At a particular temperature,the vapour pressures of two liquids $A$ and $B$ are respectively $120 \, mm$ and $180 \, mm$ of mercury. If $2 \, moles$ of $A$ and $3 \, moles$ of $B$ are mixed to form an ideal solution,the vapour pressure of the solution at the same temperature will be (in $mm$ of mercury):

Explain the terms ideal and non-ideal solutions in the light of forces of interactions operating between molecules in liquid solutions.

Liquids $A$ and $B$ form an ideal solution. At $30\,^oC$,the total vapour pressure of a solution containing $1\,mol$ of $A$ and $2\,mol$ of $B$ is $250\,mm\,Hg$. The total vapour pressure becomes $300\,mm\,Hg$ when $1$ more $mol$ of $A$ is added to the first solution. The vapour pressures of pure $A$ and $B$ at the same temperature are

Given:
Solution $A$: Phenol and aniline
Solution $B$: Chloroform and acetone
Which of the following is correct as per Raoult's law?