At 25.0 °C, the vapor pressure of pure carbon tetrachloride (CCl4) is 143. torr and the vapor pressure of pure chloroform (CHCl3) is 199 torr. The molar mass of CHCl3 is 119.38 g/mol and the molar mass for CCl4 is 154.8 g/mol. a. Do you expect the vapor pressure of a pure solvent to differ from the vapor pressure of a solution of that solvent? Why? Use the Raoult’s Law to explain. b. Calculate the vapor pressure in torr of a solution prepared by mixing 25.00 g of CCl4 and 20.00 g of CHCl3. c. Suppose you have a solution which contains CCl4 and CHCl3. Calculate the mole fraction of CHCl3 (XCHCl3) in a solution whose vapor pressure is 185. torr. Please report XCHCl3 with 3 sig figs. Recall the at 25.0 °C, the vapor pressure of pure CCl4 is 143. torr and the vapor pressure of pure chloroform (CHCl3) is 199 torr.
At 25.0 °C, the vapor pressure of pure carbon tetrachloride (CCl4) is 143. torr and the vapor pressure of pure chloroform (CHCl3) is 199 torr. The molar mass of CHCl3 is 119.38 g/mol and the molar mass for CCl4 is 154.8 g/mol. a. Do you expect the vapor pressure of a pure solvent to differ from the vapor pressure of a solution of that solvent? Why? Use the Raoult’s Law to explain. b. Calculate the vapor pressure in torr of a solution prepared by mixing 25.00 g of CCl4 and 20.00 g of CHCl3. c. Suppose you have a solution which contains CCl4 and CHCl3. Calculate the mole fraction of CHCl3 (XCHCl3) in a solution whose vapor pressure is 185. torr. Please report XCHCl3 with 3 sig figs. Recall the at 25.0 °C, the vapor pressure of pure CCl4 is 143. torr and the vapor pressure of pure chloroform (CHCl3) is 199 torr.
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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At 25.0 °C, the vapor pressure of pure carbon tetrachloride (CCl4) is 143. torr and the vapor pressure of pure chloroform (CHCl3) is 199 torr. The molar mass of CHCl3 is 119.38 g/mol and the molar mass for CCl4 is 154.8 g/mol.
a. Do you expect the vapor pressure of a pure solvent to differ from the vapor pressure of a solution of that solvent? Why? Use the Raoult’s Law to explain.
b. Calculate the vapor pressure in torr of a solution prepared by mixing 25.00 g of CCl4 and 20.00 g of CHCl3.
c. Suppose you have a solution which contains CCl4 and CHCl3. Calculate the mole fraction of CHCl3 (XCHCl3) in a solution whose vapor pressure is 185. torr. Please report XCHCl3 with 3 sig figs. Recall the at 25.0 °C, the vapor pressure of pure CCl4 is 143. torr and the vapor pressure of pure chloroform (CHCl3) is 199 torr.
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