The freezing point of 55.38 g of a pure solvent is measured to be 50.11 C. When 2.94 g of an unknown solute (assume the van 't Hoff factor = 1.0000) is added to the solvent the freezing point is measured to be 47.29 C. Answer the following questions ( the freezing point depression constant of the pure solvent is 7.25 Ckg solvent/mol solute).

What is the molality of the solution?

How many moles of solute are present?

What is the molecular weight of the solute?