At $363 \ K,$ the vapour pressure of $A$ is $21 \ kPa$ and that of $B$ is $18 \ kPa$. One mole of $A$ and $2 \ moles$ of $B$ are mixed. Assuming that this solution is ideal,the vapour pressure of the mixture is $....... \ kPa$. (Round off to the Nearest Integer).

Which of the following plots does not represent the behavior of an ideal solution of $A$ and $B$?

Two liquids $x$ and $y$ form an ideal solution. At $300 \ K$,the vapor pressure of a solution containing $1 \ mol$ of $x$ and $3 \ mol$ of $y$ is $550 \ mm \ Hg$. At the same temperature,if $1 \ mol$ of $y$ is added to the solution,the vapor pressure increases by $10 \ mm \ Hg$. The vapor pressures of pure $x$ and $y$ are respectively:

What is meant by positive and negative deviations from Raoult's law and how is the sign of $\Delta_{mix} H$ related to positive and negative deviations from Raoult's law?

Two liquids $X$ and $Y$ form an ideal solution. At $300 \ K,$ vapour pressure of the solution containing $1 \ mol$ of $X$ and $3 \ mol$ of $Y$ is $550 \ mm \ Hg.$ At the same temperature,if $1 \ mol$ of $Y$ is further added to this solution,vapour pressure of the solution increases by $10 \ mm \ Hg.$ Vapour pressure (in $mm \ Hg$) of $X$ and $Y$ in their pure states will be,respectively:

At $T \ K$,two liquids $A$ and $B$ form an ideal solution. The vapour pressures of pure liquids $A$ and $B$ at that temperature are $400 \ mm \ Hg$ and $600 \ mm \ Hg$ respectively. If the mole fraction of liquid $B$ is $0.3$ in the mixture,the mole fractions of $A$ and $B$ in the vapour phase respectively are