If the solubility of O₂ at 0.160 bar and 25°C is 6.65 g/100 g H₂O,what is the solubility of O₂ at a pressure of 1.84 bar and 25°C? A)77 g/100 g H₂O B)22.5 g/100 g H₂O C)1.7 g/100 g H₂O D)0.0 g/100 g H₂O E)0.6 g/100 g H₂O

Question

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Henry's law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. Mathematically, this can be expressed as:S = kPwhere S is the solubility of the gas in g/100 g H2O, k is the Henry's law constant, and P is the partial pressure of the gas in bar.In this problem, we are given the solubility of O2 at 0.160 bar and 25°C as 6.65 g/100 g H2O. We can use this information to find the Henry's law constant for O2:k = S/P = 6.65 g/100 g H2O / 0.160 bar = 41.56 g/100 g H2O / barNow we can use the Henry's law constant to find the solubility of O2 at a pressure of 1.84 bar and 25°C:S = kP = 41.56 g/100 g H2O / bar * 1.84 bar = 76.3 g/100 g H2OTherefore, the solubility of O2 at a pressure of 1.84 bar and 25°C is 76.3 g/100 g H2O.

If the Solubility of O2 at 0

If the Solubility of O₂ at 0