vapour pressure of chloroform and dichloromethane at 298 k are 200mm of hg and 415mm of hg respectively.

1)calculate the vapour pressure of solution prepared by mixing 25.5 g of chloroform and 40g of dichloromethane at 298K.

2)mole fraction of each component in vapour phase.

(1) Molar mass of chloroform CHCl₃ = (1 * 12) + (1 * 1) + (3 * 35.5) = 119.5 g/mol

Molar mass of dichloromethane CH₂Cl₂ = (1 * 12) + (2 * 1) + (2 * 35.5) = 85 g/mol

Moles of  CHCl₃ = 25.5/119.5 = 0.213 mol

Moles of CH₂Cl₂ = 40/85 = 0.47 mol

Total number of moles = 0.683 mol

Mole fraction of CH₂Cl₂ = 0.47/0.683 = 0.688

Mole fraction of CHCl₃ = 1 - 0.688 = 0.312

Vapor pressure of the solution can be found out using the following equation,

= 200 + (415 - 200) * 0.688

= 347 mm Hg

(2) 

Mole fraction of CH₂Cl₂ = 0.47/0.683 = 0.688

Mole fraction of CHCl₃ = 1 - 0.688 = 0.312