3. (1/2 points) Gases that are insoluble in water can be purified by bubbling th

Question

3. (1/2 points) Gases that are insoluble in water can be purified by bubbling them through water. This process removes impurities that are soluble in water. At the same time, water vapor is picked up by the sample. A sample of nitrogen that was purified by this method has a volume of 6.523 L at 26.0°C and a total pressure of 747 mmHg. In any gas sample saturated with water vapor at 26.0 the partial pressure of the water is 25.2 mmHg (a) What is the partial pressure of nitrogen in atm? (b) How many moles of nitrogen does the purified sample contain?

Explanation / Answer

a) According to dalton's lawof partial pressures, total pressure of a gas mixture is the sum of the partial pressures of the component gases ,(like N2 and water vapour)

Total Pressure =Ptotal=pN2+p(water vapour) where p=partial pressures

or,747 mmhg=pN2+25.2 mmhg

pN2=747 mmhg-25.2mmhg=721.8 mmhg

pN2 (in atm)=721.8 mmhg*(1atm/760 mmhg)=0.95 atm

b) This can be solved for mol of N2=n ,using ideal gas equation, PV=nRT

n=PV/RT

Pressure=P=0.95 atm

Volume=V=6.523L

R=ideal gas constant=0.0821L atm/K.mol

Temperature=T=26+273=299K

n=(0.95atm)*(6.523L)/(0.0821L atm/K.mol)(299K)=0.252 mol

n=0.252 mol

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