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.
Answer:
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
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