Freezing point chemistry question?

Question

Calculate the freezing points of 0.17 m glycerol in ethanol and 1.92 mol of naphthalene, C10H8, in 16.8 mol of chloroform, CHCl3. Ethanol's normal freezing point is -114.6 degrees C and molal freezing-point-depression constant (Kf) is 1.99 degrees C /m. Chloroform's normal freezing point is -63.5 degrees C and molal freezing-point-depression constant (Kf) is 4.68 degrees C/m.

Thanks!!

Answer 1

About the 1st question I can not answer because you forgot the moles of ethanol.

About the 2nd :

Mass CHCl3 = 16.8 mol x 119.378 g/mol =2005 g =>2.01 Kg

m = 1.92 / 2.01 =0.957

delta T = 4.68 x 0.957 = 4.48 °C

freezing point = - 63.5 - 4.48 =68.0 °C