A solution is prepared by dissolving 8.215 g of an unknown pure nonvolatile compound in 300.0 g of benzene (C6H6, MW = 78.11 g/mol). The freezing point of the solution is 0.38 °C lower than that of pure benzene. Based on this information, find the molecular weight of the unknown compound. Note that for benzene Tf° = 5.50 °C and Kf = 5.12 kg°C/mol.
A solution is prepared by dissolving 8.215 g of an unknown pure nonvolatile compound in 300.0 g of benzene (C6H6, MW = 78.11 g/mol). The freezing point of the solution is 0.38 °C lower than that of pure benzene. Based on this information, find the molecular weight of the unknown compound. Note that for benzene Tf° = 5.50 °C and Kf = 5.12 kg°C/mol.
Chemistry
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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
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A solution is prepared by dissolving 8.215 g of an unknown pure nonvolatile compound in 300.0 g of benzene (C6H6, MW = 78.11 g/mol). The freezing point of the solution is 0.38 °C lower than that of pure benzene. Based on this information, find the molecular weight of the unknown compound. Note that for benzene Tf° = 5.50 °C and Kf = 5.12 kg°C/mol.
Expert Solution
Step 1
Given:
Mass of compound (solute) = 8.215 g
Mass of benzene (solvent) = 300.0 g
Freezing point of pure benzene = 5.50 oC
Freezing point solution = 5.12 oC
Molal depression constant = Kf = 5.12 oC/m
Step 2
Depression in freezing point is given by:
Step 3
Calculation for molality of solution:
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