An aqueous solution is $1.00 \ molal$ in $KI$. Which change will cause the vapour pressure of the solution to increase?

The mass of glucose that should be dissolved in $100 \ g$ of water in order to produce the same relative lowering of vapour pressure as is produced by dissolving $1 \ g$ of urea (molar mass $= 60 \ g/mol$) in $50 \ g$ of water is ........... $g$. (Assume dilute solution in both cases):-

Vapour pressure of a solution of benzene $(P^o_{benzene} = 120 \ torr)$ and toluene $(P^o_{toluene} = 80 \ torr)$ having $2 \ moles$ of each is ......... $torr.$

Calculate the mole fraction of pure liquid $B$ in solution if total vapour pressure of solution,vapour pressure of pure liquid $A$ and vapour pressure of pure liquid $B$ are $500 \ mmHg$,$400 \ mmHg$ and $575 \ mmHg$ respectively at given temperature.

"The relative lowering of the vapour pressure is equal to the mole fraction of the solute." This law is called

What is the vapour pressure of a solution containing $1 \ mol$ of a non-volatile solute in $36 \ g$ of water $\left(P_1^0 = 32 \ mm \ Hg\right) (in $mm \ Hg$)?$