Using Henry's Law, Calculate percentage (by volume) of Oxygen and Nitrogen in air dissolved in water at 25C. The air in equilibrium with water at 1 bar pressure may be considered to be 20% oxygen and 80% nitrogen by volume
Henry constant for oxygen: 4.40 x 10^9 Pa
Henry constant for nitrogen: 8.68 x 10^9 PaUsing Henry's Law, Calculate percentage (by volume) of Oxygen and Nitrogen in air dissolved in water?
The solubility of oxygen in water is higher than the solubility of nitrogen.
Answer : Air dissolved in water contains approximately 35.6% oxygen compared to 21% in air.
That means the nitrogen would be about 64.4% of the air that is dissolved in the water, compared to about 79% in regular air.
--------------------------
Henry Law's Constants at a system temperature of 25C
* Oxygen - O2 : 756.7 atm/(mol/l) = 4.40 x 10^9 Pa
* Nitrogen - N2 : 1600 atm/(mol/l) = 8.68 x 10^9 Pa
-------------------------------------
Oxygen dissolved in the Water at atmospheric pressure can be calculated as:
co = (1 atm) 0.21 / (756.7 atm/(mol/liter)) (31.9988 g/mol)
= 0.0089 g/liter
-----------------------
Nitrogen dissolved in the Water at atmospheric pressure can be calculated as:
cn = (1 atm) 0.79 / (1600 atm/(mol/liter)) (28.0134 g/mol)
= 0.0138 g/liter
Subscribe to:
Post Comments (Atom)
No comments:
Post a Comment