TABLE 13.3 Molal Boiling-Point-Elevation and Freezing-Point-Depression Constants Normal Boiling Point (°C) 100.0 K, (°C/m) Normal Freezing Point (°C) K; (°C/m) Solvent Water, H2O 1.86 0.51 0.0 Benzene, C,H, 2.53 80.1 5.5 5.12 Ethanol, C,H¿OH Carbon tetrachloride, CCI4 78.4 1.22 -114.6 1.99 76.8 -22.3 29.8 5.02 Chloroform, CHCI3 4.68 61.2 3.63 -63.5
TABLE 13.3 Molal Boiling-Point-Elevation and Freezing-Point-Depression Constants Normal Boiling Point (°C) 100.0 K, (°C/m) Normal Freezing Point (°C) K; (°C/m) Solvent Water, H2O 1.86 0.51 0.0 Benzene, C,H, 2.53 80.1 5.5 5.12 Ethanol, C,H¿OH Carbon tetrachloride, CCI4 78.4 1.22 -114.6 1.99 76.8 -22.3 29.8 5.02 Chloroform, CHCI3 4.68 61.2 3.63 -63.5
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
Chapter17: Spontaneity, Entropy, And Free Energy
Section: Chapter Questions
Problem 128IP: Some nonelectrolyte solute (molar mass = 142 g/mol) was dissolved in 150. mL of a solvent (density =...
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Question
Using data from Table 13.3, calculate the freezing and boiling
points of each of the following solutions: (a) 0.22 m
glycerol (C3H8O3) in ethanol, (b) 0.240 mol of naphthalene
(C10H8) in 2.45 mol of chloroform, (c) 1.50 g NaCl
in 0.250 kg of water, (d) 2.04 g KBr and 4.82 g glucose
(C6H12O6) in 188 g of water.
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