An aqueous solution of methanol in water has a vapour pressure:

Two liquids $A$ and $B$ have vapour pressure in the ratio $P_A^o : P_B^o = 1 : 3$ at a certain temperature. If the ratio of mole fractions of $A$ to $B$ in the vapour phase is $4 : 3$,then the mole fraction of $B$ in the solution at the same temperature is

The vapour pressure of pure liquid $A$ is $0.80 \ atm$. On mixing a non-volatile solute $B$ to $A$,its vapour pressure becomes $0.6 \ atm$. The mole fraction of $B$ in the solution is

What is the vapour pressure of a solution containing $1 \ mol$ of a non-volatile solute in $36 \ g$ of water (in $mm \ Hg$)? $(P_1^0 = 400 \ mm \ Hg)$

The variation of vapour pressure $(b)$ as a function of temperature $(a)$ is studied for $C_2H_5OC_2H_5$,$CCl_4$,and $H_2O$ at $760 \ mm \ Hg$ and is shown in the figure below. The boiling temperatures of $C_2H_5OC_2H_5$,$CCl_4$,and $H_2O$ are $308 \ K$,$350 \ K$,and $373 \ K$ respectively. Curves $A$,$B$,and $C$ respectively correspond to:

$p_A$ and $p_B$ are the vapour pressures of pure liquid components $A$ and $B$ respectively of an ideal binary solution. If $x_A$ represents the mole fraction of component $A,$ the total pressure of the solution will be