
A 1.50-g sample of methanol (CH3OH) is placed in an evacuated 1.00-L container at 30 °C.
- (a) Calculate the pressure in the container if all of the methanol is vaporized. (Assume the
ideal gas law , PV = nRT.) - (b) The vapor pressure of methanol at 30 °C is 158 torr. What mass of methanol actually evaporates? Is liquid in equilibrium with vapor in the vessel?
(a)

Interpretation:
Pressure of the container has to be calculated if all the methanol present in it is vaporized.
Answer to Problem 11.95QE
The pressure of container that contains
Explanation of Solution
Mass of methanol present in the container is given as
Therefore, the number of moles present in
The ideal gas equation is given as shown below;
Rearranging the above equation in terms of pressure as follows;
Substituting the values in above equation, the pressure of container can be calculated as shown below;
Therefore, the pressure of container that contains
(b)

Interpretation:
Mass of methanol that evaporates has to be calculated and also the liquid is in equilibrium with vapor in the vessel or not has to be given.
Answer to Problem 11.95QE
The mass of vaporized methanol is
Explanation of Solution
Vapor pressure of methanol is given as
The vapor pressure of methanol can be converted into
The ideal gas equation is given as shown below;
Rearranging the above equation in terms of number of moles as follows;
Substituting the values in above equation, the number of moles of methanol can be calculated as shown below;
Therefore, the number of moles of methanol present in vapor state is
Molar mass of methanol is
Therefore, the mass of methanol is
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Chapter 11 Solutions
Chemistry: Principles and Practice
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