Question - 1) A pure solvent freezes at 12.0 deg C and a pure solute freezes at 328.0 deg C. A solution of 0.980 g of the solute and 13.870 g of the solvent freezes at 5.1 deg C. The molar mass of the solvent is 154.2 g/mol and the molar mass of the solute is 178.2 g/mol. Calculate the freezing point depression constant for the solvent.
2) A student followed our lab procedure for this experiment. He started the experiment by measuring the mass and freezing point of the pure solvent with little error. Instead of quickly finishing the experiment, he went to lunch. After returning he noted that the solvent had absorbed some impurities from the atmosphere. He went ahead and did the experiment anyway. Determine whether the measured freezing point depression in the experiement would increase, decrease, or not change compared to if the solvent has no impurities in it. Also determine whether the measured molality of the solution and the molar mass of the solute would increase, decrease, or not change.
Please illustrate work as well as walk me during the problem so that I can follow and understand it.