Qusetion: A student determined that the freezing temperature of lauric acid is 44.0 degrees celcius. When she added 1.00g of an uknown, nondissociating solute to 8.01g of lauric acid, the freezing point of the mixture went down to 39.9 degrees celcius. Lauric acid has a freezing point depression constant of 3.9 degrees celcius kg/mol.
1) calculate the freezing point depression for the mixture.
2) Calculate the molality for the solution.
3) Based on the molality of the solution and the mass of the lauric acid, how many moles of solute are present in the solution?
4) What is the molar mass of the unknown solute?
Please show all work