Chemistry partial pressures
posted by Dave .
A sample of gas collected over water at 42 degrees C occupies a volume of one liter. The wet gas has a pressure of .986 atm. The gas is dried and the dry gas occupies 1.04 L with a pressure of 1.00 atm at 90 degrees C. Using this information, calculate the vapor pressure of water at 42 degrees C.
I was going to approach this problem by finding the pressure of the gas when dry at 42 degrees C, and then do
P[dry]= P[total]  P[water pressure]
but I realized this would get me nowhere as I didn't know the total pressure. Is there a better way to do this problem?
Calculate total mols H2O and gas @ 42^{o} C from PV = nRT.
Calculate mols dry gas from the second set of conditions @ 90^{o} C.
The difference in mols should be the mols H2O vapor and that put back into the PV=nRT at 42 should give P of water at 42.
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