The solubility of nitrogen gas in water at 25°C and a nitrogen pressure of 522 mmHg is 4.7 × 10^-4 mol/L. What is the value of the Henry's law constant in mol L^-1• atm^-1? A) 6.8 × 10^-4 mol L^-1• atm^-1 B) 4.7 × 10^-4 mol L^-1• atm^-1 C) 3.2 × 10^-4 mol L^-1• atm^-1 D) 9.0 × 10^-7 mol L^-1• atm^-1 E) 1.5 × 10³ mol L^-1• atm^-1

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Quizplus · Accepted Answer

Henry's law states that the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid. The constant of proportionality is known as Henry's law constant (kH). The formula for Henry's law is S = kH * P, where S is the solubility of the gas, kH is Henry's law constant, and P is the pressure of the gas.Given:- Solubility (S) = 4.7 × 10^-4 mol/L- Pressure (P) = 522 mmHg = 522/760 atm (since 1 atm = 760 mmHg)To find kH, rearrange the formula to kH = S / P.kH = (4.7 × 10^-4 mol/L) / (522/760 atm) = (4.7 × 10^-4 mol/L) / (0.6868 atm) ≈ 6.8 × 10^-4 mol/L•atmTherefore, the Henry's law constant is 6.8 × 10^-4 mol/L•atm.

The Solubility of Nitrogen Gas in Water at 25°C and a Nitrogen