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Pure iodine (102 g) is dissolved in 325 g of CCl4 at 65 °C. Given that the vapor pressure of CCl4 at this temperature is 531 mm Hg, what is the vapor pressure of the CC14-12 solution at 65 °C? (Assume that I2 does not contribute to the vapor pressure.) Vapor pressure = mm Hg

Pure iodine (102 g) is dissolved in 325 g of CCl4 at 65 °C. Given that the vapor pressure of CCl4 at this temperature is 531 mm Hg, what is the vapor pressure of the CC14-12 solution at 65 °C? (Assume that I2 does not contribute to the vapor pressure.) Vapor pressure = mm Hg

Chemistry
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
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Pure iodine (102 g) is dissolved in 325 g of CCl4 at 65 °C. Given that the vapor pressure of CC14 at this temperature is 531 mm Hg, what is the vapor pressure of the CC14-12 solution at 65 °C? (Assume that I2 does not contribute to the vapor pressure.) Vapor pressure = mm Hg
Transcribed Image Text:Pure iodine (102 g) is dissolved in 325 g of CCl4 at 65 °C. Given that the vapor pressure of CC14 at this temperature is 531 mm Hg, what is the vapor pressure of the CC14-12 solution at 65 °C? (Assume that I2 does not contribute to the vapor pressure.) Vapor pressure = mm Hg
Expert Solution
Step 1

Molecular weight of I2 = 253.81 g/mol

Number of moles of non-volatile solute (I2) = mass/mol.wt. = 102 g/(253.81 g/mol)= 0.40188 mol

Mass of CCl4 = 325 g

Molecular weight of CCl4 = 153.82 g/mol

Number of moles of solvent water = 325 g/(153.82 g/mol) = 2.11286 mol

Total number of moles = 0.40188 + 2.11286 = 2.51473 mol

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