If air contains 78%N2 by volume ,what is the solubility of nitrogen in water at 25°©?

Answer 1

<<Henry's law:
[N₂] = kH ∙ p(N₂)

Assuming ideal gas mixture the partial pressure of nitrogen equals 78% of the total pressure, i.e.
p(N₂) = 0.78 atm

So the solubility of nitrogen under these conditions is:
[N₂] = 7×10⁻⁴mol/(Latm) ∙ 0.78 = 5.46×10⁻⁴mol/L >>

Answer 2

%V is given. How it could be compared as partial pressure?

Answer 3

Thank

Answer 4

10Q

Answer 5

what happen to the Atm in the problem?

Answer 6

P Thompson atm given in the question is total pressure and with the help of that we have to find partial pressure

Answer 7

Seidaddis421

Answer 8

5.46×10^-4mol/l

Answer 9

Is Henry's constant the same at 20°c and 25°c???

Answer 10

No the Henry's constant is only at 25 c°