The solubility of pure Nitrogen gas at 25C and 1atm is 6.8*10^-4mol/L. What is the concentration of Nitrogen dissolved in water under atmospheric conditions? The partial pressure of Nitrogen gas in atmosphere is 0.78atm

Since in this problem ‘k’ is not given so we have to find out.

Applying Henry’s equation,S = k P

k= S/P = 6.8 X 10^-4 mol L^-1  =   6.8 X 10^-4 mol L^-1 

                            1

 So the solubility of N₂ at 0.78 atm:

S= (6.8 X 10^-4 mol L^-1 ) (0.78 atm) = 5.3 x10^-4 M

Since in this problem ‘k’ is not given so we have to find out.

S = k P

k= S/P = 6.8 X 10^-4 mol L^-1  =   6.8 X 10^-4 mol L^-1 

                            1

 So the solubility of N₂ at 0.78 atm:

S= (6.8 X 10^-4 mol L^-1 ) (0.78 atm) = 5.3 x10^-4 M

Since in this problem ‘k’ is not given so we have to find out.

Applying Henry’s equation,S = k P

k= S/P = 6.8 X 10^-4 mol L^-1  =   6.8 X 10^-4 mol L^-1 

                            1

 So the solubility of N₂ at 0.78 atm:

S= (6.8 X 10^-4 mol L^-1 ) (0.78 atm) = 5.3 x10^-4 M