The vapor pressure of ethanol, C2H5OH, at 20 oC is 400 mmHg. Suppose that 6.5 grams...
The vapor pressure of ethanol, C2H5OH, at 20 oC is 400 mmHg. Suppose that 6.5 grams of it are sealed in a 15.0-liter flask. Determine the mass of ethanol that enters the gas phase and the amount that remains in the liquid state upon equilibrium being established.
Homework Answers
Let n moles of Ethanol evaporate
So, Using Ideal gas Law
PV = nRT
P= 400mmHg = 400/760 atm = 0.526 atm
T = 20C = 293K
R = 0.0821 atmL/mol.K
V = 15L
n = PV/RT
=( 0.526*15)/(0.0821*293)
=0.328 moles
Molar mass of ethanol = 46g/mol
So mass of Ethanol evaporated = 46*0.328 = 15.08 g
But we have only 6.5g
So this means that all the ethanol will vaporize to gas phase.
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figure 1
Figure 2
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figure 1
Figure 2
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