(a) Calculate the elevation of boiling point of a solution when 3 g of CaCl_2(. Molar mass.=111 g mol^-1) was dissolved in 260 g of water, assuming…

Calculate the elevation of boiling point of a solution when $\displaystyle 3$ g of $\displaystyle \mathrm{CaCl}_{2}\left(\right.$ Molar mass $\displaystyle \left.=111 \mathrm{~g} \mathrm{~mol}^{-1}\right)$ was dissolved in $\displaystyle 260$ g of water, assuming that $\displaystyle \mathrm{CaCl}_{2}$ undergoes complete dissociation. ( $\displaystyle \mathrm{K}_{\mathrm{b}}$ for water $\displaystyle =0.52 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$ )

Liquids 'X' and 'Y' form an ideal solution. The vapour pressure of pure 'X' and pure 'Y' are $\displaystyle 120$ mm Hg and $\displaystyle 160$ mm Hg respectively. Calculate the vapour pressure of the solution containing equal moles of 'X' and 'Y'.