Answer to Question #187993 in General Chemistry for Ace

Question

Camphor (C10H16O2) freezes at 175 °C, and it has a particularly large freezingpoint-depression constant, Kf = 40.0 °C/m. When 0.086 g of an organic substance of unknown molar mass is dissolved in 22.01 g of liquid camphor, the freezing point of the mixture is found to be 1.7 °C below of pure camphor. What is the molar mass of the solute?

You add 0.25 g of an unknown solute to 11.1 g of benzene. The boiling point of the benzene rises from 80.10 °C to 80.46 °C. What is the molar mass of the compound? Kb=2.53 °C /m 

A solution of an unknown non-dissociating solute was prepared by dissolving 0.300 g of the substance in 40.0 g of CCl4. The boiling point of the solution was 0.357 °C higher than that of the pure solvent. Calculate the molar mass of the solute. Kb=5.02 °C/m

Answer 1

Molar mass of the solute=4.55M

molar mass of the compound=3.47M