Sketch a T x y diagram and label the liquid, vapour and liquid-vapour regions as well as the bubble and dew curves

Calculate the excess volume for the propanol(1)/water(2) mixture with a mole fraction of 0.16656 propanol at $25^\circ\mathrm{C}$ if the mixture's volume is $27.016\ \mathrm{cm^3\,mol^{-1}}$. The volume for propanol and water at $25^\circ\mathrm{C}$ are $75.168\ \mathrm{cm^3\,mol^{-1}}$ and $18.068\ \mathrm{cm^3\,mol^{-1}}$ respectively.

Calculate the pressure required to hold the chloroform(1)/methanol(2) system in vapour-liquid equilibrium at $36^\circ\mathrm{C}$ if the mole fractions of chloroform in the liquid and vapour phase are 0.44 and 0.657 respectively. The activity coefficients are $\gamma_1 = 1.6423$ and $\gamma_2 = 0.9534$ and the saturation pressures can be found using the Antoine equations below: $\ln P^{sat}_{Chloroform}/\mathrm{kPa} = 13.7324 - \dfrac{2548.74}{T/^\circ\mathrm{C} + 218.552}$ $\ln P^{sat}_{Methanol}/\mathrm{kPa} = 16.5785 - \dfrac{3638.27}{T/^\circ\mathrm{C} + 239.500}$

The cracking of pure n-butane via the reaction below is performed at 750 K, where the equilibrium constant, $K$, for the reaction is 6.0. $C_4H_{10} \rightarrow C_2H_4 + C_2H_6$ Calculate the mole fractions for all species if the reaction starts from 1 mole of C4H10 and is carried out in the gas phase where the pressure is 2 bar and standard pressure is 1 bar. You can assume all species are ideal gasses.