If N2 gas is bubbled through water at 293 K, how many milli moles of N2 gas would dissolve in 1 litre of water. Assume that N2 exerts a partial pressure of 0.987 bar. The KH for N2 at 293 K is 76.48 k bar.

If N2 gas is bubbled through water at 293 K, how many milli moles of N2 gas would dissolve in 1 litre of water. Assume that N2 exerts a partial pressure of 0.987 bar. The KH for N2 at 293 K is 76.48 k bar.

Given Values

Pgas = 0.987 bar

KH = 76.48 Kbar = 76480 bar

VSol ≈ VWater = 1 L or 1000 mL

Dwater = 1 gm/mL

∴  WWater = 1000 gm

MWater = 2(1)+16 = 18

Calculations

Calculate moles of Nitrogen gas:

$$n_{B}=\frac{P_{gas} \times W_{A}}{M_{A} \times K_{H}}$$

$$n_{B}=\frac{0.987~bar \times 1000~gm}{18~gm/mol \times 76480~bar}$$

nB = 0.71 × 10–3 moles

OR

nB = 0.71 millimoles