Answer Happy

Boiling Point Elevation/Freezing Point Depression ΔT=mK Where: ΔT=T (solution) −T (pure solvent) ∗ m= (\# moles solute / Kg solvent) Kb​= boiling point elevation constant. Kf​= freezing point depression constant. Kb​ and Kf​ depend only on the SOLVENT. Below are some common values. Use these values for the calculations that follow.
Use the References to access important values if needed for this question. The freezing point of water, H2​O, is 0.000∘C at 1 atmosphere. Kf​( water )= −1.86∘C/m In a laboratory experiment, students synthesized a new compound and found that when 12.27 grams of the compound were dissolved in 275.0 grams of water, the solution began to freeze at −0.242∘C. The compound was also found to be nonvolatile and a non-electrolyte. What is the molecular weight they determined for this compound ? g/mol
Use the References to access important values if needed for this question. The freezing point of benzene, C6​H6​, is 5.500∘C at 1 atmosphere. Kf​( benzene )=−5.12∘C/m In a laboratory experiment, students synthesized a new compound and found that when 10.47 grams of the compound were dissolved in 270.4 grams of benzene, the solution began to freeze at 4.813∘C. The compound was also found to be nonvolatile and a non-electrolyte. What is the molecular weight they determined for this compound ? m/mol