The solubility of nitrogen gas 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·atm? A)6.8 * 10^-4 mol/L·atm B)4.7 * 10^-4 mol/L·atm C)3.2 * 10^-4 mol/L·atm D)9.0 * 10^-7 mol/L·atm E)1.5 * 10³ mol/L·atm

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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 is calculated as solubility/pressure. Convert 522 mmHg to atm (522 mmHg / 760 mmHg/atm = 0.6868 atm), then divide the solubility (4.7 * 10^-4 mol/L) by the pressure in atm (0.6868 atm) to get approximately 6.8 * 10^-4 mol/L·atm.

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