Problem: In a system for separating gases a tank containing a mixture of hydrogen and carbon dioxide is connected to a much larger tank where the pressure is kept very low. The two tanks are separated by a porous membrane through which the molecules must effuse. If the initial partial pressures of each gas is 5.00 atm, what will be the mole fraction of hydrogen in the tank after the partial pressure of carbon dioxide has declined to 4.50 atm?

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FREE Expert Solution

Recall that Graham's Law of Effusion allows us to compare the rate of effusion of two gases


rateH2rateCO2=MMCO2MMH2rateH2rateCO2=44.0 g/mol2.0 g/molrateH2rateCO2=4.69rateH2=4.69(rateCO2)

rate=change in concentrationchange in time=moles (n)volume (V)t   rateH2rateCO2=[nV·t]H2[nV·t]CO2=[PRT]H2[PRT]CO2   recall that: PV=nRT PRT=nVrateH2rateCO2=PH2PCO2=4.69PH2=4.69PCO2


Ptotal=PCO2,f+PH2,f  χH2=nH2ntot=PH2,fPtot

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Problem Details

In a system for separating gases a tank containing a mixture of hydrogen and carbon dioxide is connected to a much larger tank where the pressure is kept very low. The two tanks are separated by a porous membrane through which the molecules must effuse. If the initial partial pressures of each gas is 5.00 atm, what will be the mole fraction of hydrogen in the tank after the partial pressure of carbon dioxide has declined to 4.50 atm?

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

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Based on our data, we think this problem is relevant for Professor Bliem's class at UNC.