QuestionDetails: Nitrogen is dissolved in water with the total pressure of gas(N

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QuestionDetails: Nitrogen is dissolved in water with the total pressure of gas(Nitrogen + water vapor) over the water being 1.40 atm. Thetemperature is 25o C.

What is the concentration of Nitrogen in the water? Give youranswer in g/L .


The vapor pressure of water at 25.0oC is 23.8 mmHg. QuestionDetails: Nitrogen is dissolved in water with the total pressure of gas(Nitrogen + water vapor) over the water being 1.40 atm. Thetemperature is 25o C.

What is the concentration of Nitrogen in the water? Give youranswer in g/L .


The vapor pressure of water at 25.0oC is 23.8 mmHg. QuestionDetails: Nitrogen is dissolved in water with the total pressure of gas(Nitrogen + water vapor) over the water being 1.40 atm. Thetemperature is 25o C.

What is the concentration of Nitrogen in the water? Give youranswer in g/L .


The vapor pressure of water at 25.0oC is 23.8 mmHg.

Explanation / Answer

The partial pressure of nitrogen is given byDalton's law
p(N2) = p - p(H2O) = 1.40 atm- 23.8/760 atm = 1.3687 atm
(Note 1atm = 760Torr = 760mmHg)

To calculate the vapor liquid equilibrium you need theHenry-constant of Nitrogen at 25°C. In terms of liquid phaseconcentration and partial pressure it is :
kH = c(N2) / p(N2) = 6.1·10?4(mol/(L·atm)
Therefore the liquid phase concentration is:
c(N2) = kH ·p(N2) = 6.1·10?4mol/(L·atm)·1.3687 atm= 0.000834907 mol/L
To obtain the mass concentration just multiply with Molar mass ofNitrogen
(N2) =c(N2)·M(N2) = 0.000834907 mol/L·28g/mol =0.02338 g/L hope this helps.......... hope this helps..........

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