A cylinder containing ethanol is submitted to a certain pressure. At a temperature of 273 K, when the applied pressure is 1.0 atm, the vapor pressure of the ethanol is 1.25 kPa. Considering that the molar volume of ethanol at 273 K is 1.22 x 10-2 dm3/mol, calculate the vapor pressure of ethanol when the pressure on the liquid reaches 4.00 MP
A cylinder containing ethanol is submitted to a certain pressure. At a temperature of 273 K, when the applied pressure is 1.0 atm, the vapor pressure of the ethanol is 1.25 kPa. Considering that the molar volume of ethanol at 273 K is 1.22 x 10-2 dm3/mol, calculate the vapor pressure of ethanol when the pressure on the liquid reaches 4.00 MP
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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A cylinder containing ethanol is submitted to a certain pressure. At a temperature of 273 K, when the applied pressure is 1.0 atm, the vapor pressure of the ethanol is 1.25 kPa. Considering that the molar volume of ethanol at 273 K is 1.22 x 10-2 dm3/mol,
calculate the vapor pressure of ethanol when the pressure on the liquid reaches 4.00 MPa.
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