At $27^{\circ} C$,two liquids $A$ and $B$ form an ideal solution with mole fractions $0.67$ and $0.33$ respectively. If the vapour pressure of pure $A$ and $B$ at $27^{\circ} C$ are $300 \ mm$ and $450 \ mm$ respectively,the total vapour pressure of the solution in $mm$ is:

Identify the mixture that shows positive deviations from Raoult's Law.

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

$2 \ moles$ each of liquids $A$ and $B$ are dissolved to form an ideal solution. What will be the mole fraction of $B$ in the vapour phase? Given: $P_A^o = 120 \ torr, P_B^o = 80 \ torr$

Benzene and toluene form an ideal solution. If the partial vapor pressures of benzene and toluene are $1.55 \ kPa$ and $1.85 \ kPa$ respectively,what is the mole ratio of benzene to toluene in the solution?

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