For an ideal solution of two components $A$ and $B$,which of the following is true?

If liquids $A$ and $B$ form an ideal solution,which of the following statements is true?

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).

At $300 \ K$,the vapour pressures of $A$ and $B$ liquids are $500 \ mm \ Hg$ and $400 \ mm \ Hg$ respectively. Equal moles of $A$ and $B$ are mixed to form an ideal solution. The mole fraction of $A$ and $B$ in the vapor state is respectively:

Liquids $A$ and $B$ form an ideal solution over the entire range of composition. At temperature $T$,an equimolar binary solution of liquids $A$ and $B$ has a vapour pressure of $45 \ Torr$. At the same temperature,a new solution of $A$ and $B$ having mole fractions $x_A$ and $x_B$,respectively,has a vapour pressure of $22.5 \ Torr$. The value of $x_A / x_B$ in the new solution is . . . . . (Given that the vapour pressure of pure liquid $A$ is $20 \ Torr$ at temperature $T$)

When acetone is added to chloroform,then a hydrogen bond is formed between them. These liquids show: