The vapour pressure of pure benzene and toluene are $160$ $mm \ Hg$ and $60$ $mm \ Hg$ respectively. The mole fraction of benzene in the vapour phase in contact with an equimolar solution of benzene and toluene is:

Which one of the following represents the graph between $\log p$ (on $Y$-axis) and $\frac{1}{T}$ (on $X$-axis)?
($p=$ vapour pressure of a liquid, $T=$ absolute temperature)

Which of the following statements is incorrect?

At $25\,^oC$,the vapour pressure of pure liquid $A$ (mol. wt. $= 40$) is $100\,torr$,while that of pure liquid $B$ is $40\,torr$ (mol. wt. $= 80$). The vapour pressure at $25\,^oC$ of a solution containing $20\,g$ of each $A$ and $B$ is ........... $torr$.

At $T \ K$,the vapour pressure of an aqueous solution of a non-volatile solute,whose mole fraction is $0.02$,is found to be $34.65 \ mm \ Hg$. What is the vapour pressure (in $mm \ Hg$) of pure water at the same temperature?

What is the relationship between vapor pressure and temperature? What will be the vapor pressure at $373 \, K$?