In a mixture of $A$ and $B$ components,the solution shows negative deviation when:

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

Formation of a solution from two components can be considered as
$(i)$ Pure solvent $\to$ separated solvent molecules $\Delta H_1$
$(ii)$ Pure solute $\to$ separated solute molecules $\Delta H_2$
$(iii)$ Separated solvent and solute molecules $\to$ solution $\Delta H_3$
Solution so formed will be ideal if

Which of the following are correct for an ideal solution?
$(a) \Delta V_{\text{mix}} = 0$
$(b) V_{\text{solvent}} + V_{\text{solute}} = V_{\text{solution}}$
$(c) \Delta H_{\text{mix}} = 0$
$(d) H_2O + CO_2 \rightarrow H_2CO_3$ is an example of an ideal solution.

At $88 \, ^\circ C$,the vapor pressure of benzene is $900 \, \text{torr}$ and the vapor pressure of toluene is $360 \, \text{torr}$. What is the mole fraction of benzene in the mixture with toluene at $1 \, \text{atm}$ and $88 \, ^\circ C$? Assume benzene and toluene form an ideal solution.

Assuming the formation of an ideal solution,determine the boiling point of a mixture containing $1560 \ g$ benzene (molar mass $= 78 \ g/mol$) and $1125 \ g$ chlorobenzene (molar mass $= 112.5 \ g/mol$) against an external pressure of $1000 \ torr$. Use the provided vapor pressure vs. temperature graph to find the answer. (in $^{\circ}C$)