c.)?

The following table gives the vapor pressure of chloroform in equilibrium with liquid chloroform(1) + acetone(2) solutions at 35 C. Xi pi/kPa 0 0 0.0603 1.26 0.1853 4.25 0.2910 7.39 HL a) Use this data to calculate the Henry's law constant k, for the solute chloroform(1) in the solvent acetone(2) at 35 C. Suggestion: prepare a graph of pi plotted against XI. b) Calculate the Henry's law activity coefficient nl for chloroform in the solution with x1 = 0.2910. c) The Henry's law constant k, for chloroform is significantly lower than the vapor pressure of pure chloroform (p*= 39.1 kPa at 35 C). Why? Give a molecular explanation. Hint ki measures the escaping tendency of chloroform molecules from liquid acetone, whereas pemeasures the escaping tendency of chloroform molecules from liquid chloroform