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When 10.83 g of glucose was dissolved in 109.6 g of benzene, the freezing point was...

When 10.83 g of glucose was dissolved in 109.6 g of benzene, the freezing point was 275.8 K. What is the formula mass of this compound? The freezing point depression constant for benzene is 5.12 (°C*kg)/mol. The melting point and boiling points are 5.50°C and 80.10°C, respectively. Aren't only I able to obtain formula mass of glucose?

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Answer #1
  1. Determine the change in freezing point from the observed freezing point of the solution and the freezing point of the pure solvent. (This will be a negative number.)

  2. Determine the molal concentration, m, from the change in freezing point and the freezing point depression constant.

  3. Determine the moles of unknown (the solute) from the molality of the solution and the mass of solvent (in kilograms) used to make the solution.

  4. Determine the molar mass from the mass of the unknown and the number of moles of unknown.

putting the value you could easily get the result

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