Question

At a certain temperature the vapor pressure of pure chloroform (CHCI3) is measured to be 0.30 atm. Suppose a solution is prepared by mixing 128. g of chloroform and 76.1 g of heptane (C7H16). Calculate the partial pressure of chloroform vapor above this solution. Be sure your answer has the correct number of significant digits. Note for advanced students: you may assume the solution is ideal. atm x 5 ?

Answer 1

- Ansvar: Amount of chloroform = 128.09 Molar mass of chloroform = 119,5 g/mol Moles of chiloroforma 128.09 1 .071 mol = n, 119.5g/mol Amount of heptane = 7.61 g Molar mass of heptane loogland Moles of heptane = 76.1g = 0.761 mol = 12. Too gland Mole fraction of chloroforma = 10071 mol = 0.5846 1.071 mol +0.761 mil Vapor pressure of chloroforma Mole fraction X Vaper pressure of pure chloroform Valper pressure of pure chloroform. 0.30 atm. Napor pressure of chloroform= 0.5846 x 0.30 atm = 0.17538 atn. = 0.18 atm - In correct a significant figures