The freezing point of a solution that contains 1.1 g of an unknown compound, (A),dissolved in 12 g of benzene is found to be 2.97 °C.The freezing point of pure benzene is 5.48 °C. The freezing point depression constantof benzene is 5.12 °C/molal. What is the molecular weight of the unknowncompound?

The freezing point of solvent decreases on addition of non volatile solute as the solute occupies…

Answered: The freezing point of a solution that…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The initial freezing temperature of 0.13 kg of a pure solvent is 6°C. 15.0 grams of a solute with molar mass of 147.63 g/mol is added to the pure solvent. The solute is known to dissociate into 2 ionic particles when dissolved in the pure solvent. The freezing temperature of the solution after the addition of the solute is -3°C. What is the Kf of the solvent?
When 397.g of benzamide C7H7NO are dissolved in 1400.g of a certain mystery liquid X, the freezing point of the solution is 4.8°C lower than the freezing point of pure X. On the other hand, when 397.g of iron(III) chloride are dissolved in the same mass of X, the freezing point of the solution is 11.8°C lower than the freezing point of pure X.Calculate the van't Hoff factor for iron(III) chloride in X. Be sure your answer has a unit symbol, if necessary, and round your answer to 2 significant digits. i=
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