Open Question
At 298 K, the Henry's law constant for oxygen is 0.00130 M/atm. Air is 21.0% oxygen. At 298 K, what is the solubility of oxygen in water exposed to air at 1.00 atm?
14. Solutions
Henry's Law Calculations
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At 25 degrees Celsius, the Henry's Law constant for hydrogen sulfide (H2S) gas in water is 0.087 M/atm. Calculate the mass in grams of the gas that can be dissolved in 700 mL of water at 25 degrees Celsius and a partial pressure of 1.79 atm.
A
3.60 grams
B
7.89 grams
C
5.12 grams
D
3.45 grams
Verified step by step guidance1
Start by understanding Henry's Law, which states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. The formula is: , where is the concentration of the gas, is the Henry's Law constant, and is the partial pressure.
Calculate the concentration of hydrogen sulfide in water using Henry's Law. Substitute the given values into the formula: .
Convert the volume of water from milliliters to liters, as the concentration calculated will be in molarity (moles per liter). Use the conversion: .
Calculate the number of moles of hydrogen sulfide dissolved in the water using the concentration and volume: , where is the volume in liters.
Convert the moles of hydrogen sulfide to grams using its molar mass. The molar mass of H2S is approximately 34.08 g/mol. Use the formula: .
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