Problem: The vapor pressure of ethanol (C2H5OH) at 19˚C is 40.0 torr. A 0.900-g sample of ethanol is placed in a 2.80 L container at 19˚C. If the container is closed and the ethanol is allowed to reach equilibrium with its vapor, how many grams of liquid ethanol remain?

FREE Expert Solution

 Calculate the mass of gas present in the container using the ideal gas equation.

PV=nRT

P = pressure, atm
V = volume, L
n = moles, mol
R = gas constant = 0.08206 (L·atm)/(mol·K)
T = temperature, K


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Problem Details

The vapor pressure of ethanol (C2H5OH) at 19˚C is 40.0 torr. A 0.900-g sample of ethanol is placed in a 2.80 L container at 19˚C. If the container is closed and the ethanol is allowed to reach equilibrium with its vapor, how many grams of liquid ethanol remain?

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Our tutors have indicated that to solve this problem you will need to apply the The Ideal Gas Law concept. You can view video lessons to learn The Ideal Gas Law. Or if you need more The Ideal Gas Law practice, you can also practice The Ideal Gas Law practice problems.

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