The freezing point of CCl4 is -22.92°C. Calculate the freezing point of the solution prepared by dissolving 17.5g of pyrazine (C4H4N2) in 1250g of CCl4. The freezing point depression constant for CCl4 is 29.8 °C/m.

If the freezing point of the solution was observed to be -8.6 °C, and the normal freezing point of cyclohexane is 6.50 °C, what is the value of Kf for cyclohexane? 4.67 g of toluene in 67.8 g of cyclohexane The molar mass of toluene is 92.14 g/mol.

Calculate the molality of a solution formed by adding 2.60 g NHCl to 19.1 g of water. molality: m NH₂Cl

None

Calculate the freezing point of a solution that contains 168.4 g of sucrose (table sugar) in 300. g of water. One mole of sucrose is 342 g. Kf for H2O = 1.86°C/m -0.185 oC -3.05 oC -0.558 oC -0.744 oC -1.24 oC

The freezing point of CCI4 is -22.3°C and the freezing point depression constant is 29.8 °C/m. If a solution of C5H12 in CCI4 freezes at -37.6°C, what is the molality of this solution? O 0.513 0.722 O 2.01 O 5.01 O 1.26

The freezing point of an aqueous solution containing 35 g of an nonelectrolyte in 150 mL water is -10.4ï°C. What is the molecular weight of the compound? Kf = 1.86°C/m for water.     121 g/mol     2.78 g/mol     34.4 g/mol     41.73 g/mol     53.8 g/mol