Solubility of H2S gas = 0.195 m
= 0.195 mole in 1 kg of the Solvent (water)
1 kg of the solvent (water) = 1000 g = \(\frac{1000\,g}{18\,g\,mol^{-1}}\) = 55.55 moles
Mole fraction of H2S gas in the solution (x) = \(\frac{0.195}{0.195+55.55}\) = 0.0035
Pressure at STP = 0.98 7 bar
Applying Henry’s law
\(P_{H_2S}=K_H\times x_{H_2S}\)