due soon please with explnation

Instructor's initials 4. If 2.15g of an unknown solid nonclectrolyte is dissolved in 18.6g of naphthalene, the the freezing point depression constant for to freeze 4.3C lower than pure naphthalene. If following. a. The molality of the solution by using only the freezing point depression and the freezing point depression constant. b. The number of moles of unknown dissolved in the 18.6g of naphthalene using the mass of naphthalene and the molality of the unknown. c. The molar mass of the unknown. d. The molecular formula of the unknown if it is comprised of 40.0% carbon, 6.7% hydrogen and 53.3% oxygen. 1. Solutions a. What is the solid that forms when a solution starts to freere? b. Will your answer for part a of this question be correct for all solutions that use solvents that are liquids at room temperature? Explnin. 2. Freezing points a. Compare the temperature change as a pure liquid is converted to a solid at its freezing point with the temperature change as a solution is converted to a solid at its freezing? b. Explain how your answer to part a. of the question is related to the equation given at the end of the Introduction to this Experiment. 3. If you weigh the lauric acid to the nearest 0.1g and you weigh the unknown solid to the nearest 0.0001g, can you calculate a molar mass (molecular weight) of your unknown solid to three significant figures? Show your reasoning. PartMassDatoforLiuinoAcitMawofteuttube(c)Massoftesttubeandlauricaeld(n)/6.234 TABCE 2. Temperature-Time Data for Cooling Puro Lauric Acid. Sample Calculations Freezing point depression, dTf Molality of unknown, m Moles of unknown Molar Muss of unknown Instructor's initials