At 25°c the henry's law constant for nitrogen trifluoride (nf3) gas in water is 7.9 × 10-4 m/atm. what is the mass of nf3 gas that can be dissolved in 150 ml of water at 25°c and an nf3 partial pressure of 1.71 atm?

For this problem, we should use the Henry's Law formula which is written below:

P = kC
where
P is the partial pressure of the gas
k is the Henry's Law constant at a certain temperature
C is the concentration

Substituting the values,
1.71 atm = (7.9×10⁻⁴ /atm)C
Solving for C,
C = 2164.56 molal or 2164.56 mol/kgwater

Let's make use of density of water (1 kg/1 m³) and the molar mass of NF₃ (71 g/mol).

Mass of NF₃ = 2164.56 mol/kg water * 1 kg/1 m³ * 1 m³/1000000 mL * 150 mL * 71 g/mol = 23.05 g 

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