K _ H for O ₂ at 293 ~K is 34.86 ~kbar . What should be the partial pressure of O ₂ gas so that it has a solubility of 0.08 ~g / L in water at 293 ~K ? (Density of solution =1 ~g / ml )

Step-by-step solution

Henry's Law states that P = K_ H x , where P is the partial pressure of the gas, K_ H is Henry's constant, and x is the mole fraction of the gas in the solution. Given solubility of O₂ = 0.08 g/L . The molar mass of O₂ is 32 g/mol . Number of moles of O₂ in 1 L of solution = 0.08 g 32 g/mol = 0.0025 mol . Density of solution = 1 g/mL = 1000 g/L . Mass of 1 L of solution = 1000 g . Assuming the solution is dilute, the mass of water in 1 L is approximately 1000 g . Number of moles of water = 1000 g 18 g/mol 55.55 mol