The solubility of nitrogen gas in water at 25°c and a nitrogen pressure of 522 mm hg is 4.7 × 10⁻⁴ mol/l. what is the value of the henry's law constant in mol l⁻¹• atm⁻¹?
a. 9.0 x 10⁷ mol/l atm
b. 3.2 x 10⁻⁴ mol/l atm
c. 4.7 x 10⁻⁴ mol/l atm
d. 6.8 x 10⁻⁴ mol/l atm
e. 1.5 x 10³ mol/l atm

D. 6.8 x 10⁻⁴ mol/L atm

Explanation:

Henry's Law states that:

S = kH * P

Where S is the solubility of a gas (in mol/L), kH is Henry's constant (in mol• L⁻¹• atm⁻¹) and P is the partial pressure of said gas (in atm).

The problem gives us S and P, while asking us to calculate kH:

Now we solve for kH:

4.7 × 10⁻⁴ mol/L = kH * 0.687 atm