A solution containing 0.10 mol of naphthalene (nonvolatile) and 0.90 mol of benzene is cooled until some solid benzene freezes out. The solution is then decanted off from the solid and the decanted solution is warmed to 80°C, at which temperature the vapor pressure above the solution is found to be 670 torr. The normal freezing and boiling points of pure benzene are 5.5 °C and 80°C, respectively and the molar enthalpy of fusion of benzene ∆fus?=10.67 kJ/mol Assume the solution is ideal. a) Calculate the temperature to which the solution was cooled originally. b) Calculate the number of moles of benzene that froze out.
A solution containing 0.10 mol of naphthalene (nonvolatile) and 0.90 mol of benzene is cooled until some solid benzene freezes out. The solution is then decanted off from the solid and the decanted solution is warmed to 80°C, at which temperature the vapor pressure above the solution is found to be 670 torr. The normal freezing and boiling points of pure benzene are 5.5 °C and 80°C, respectively and the molar enthalpy of fusion of benzene ∆fus?=10.67 kJ/mol Assume the solution is ideal. a) Calculate the temperature to which the solution was cooled originally. b) Calculate the number of moles of benzene that froze out.
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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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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A solution containing 0.10 mol of naphthalene (nonvolatile) and 0.90 mol of benzene is cooled until some solid benzene freezes out. The solution is then decanted off from the solid and the decanted solution is warmed to 80°C, at which temperature the vapor pressure above the solution is found to be 670 torr. The normal freezing and boiling points of pure benzene are 5.5 °C and 80°C, respectively and the molar enthalpy of fusion of benzene ∆fus?=10.67 kJ/mol Assume the solution is ideal.
a) Calculate the temperature to which the solution was cooled originally.
b) Calculate the number of moles of benzene that froze out.
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