A 0.756 g sample of an unknown nonelectrolyte is dissolved in 11.451 g of benzophenone and produces a solution that freezes at 45.2 degrees C. If pure benzophenone melted at 48.0 degrees C, what is the molecular weight of the compound? I am familiar with the formula but I am confused with whether to use molality or molarity and how to calculate it.
Tf = i*Kf *m
i = 1 for non electrolyte
Kf = 9.80C/m
Tf = 48-45.2 = 2.80C
Tf = i*Kf *m
2.8 = 1*9.8*m
m = 2.8/9.8 = 0.286m
molality = W*1000/G.M.Wt * weight of solvent in g
0.286 = 0.756*1000/G.M.Wt*11.451
G.M.Wt = 0.756*1000/0.286*11.451 = 230.84g/mole
molar mass of unknown = 230.84g/mole
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