Open Question
Calculate the mass of nitrogen dissolved at room temperature in an 80.0-L home aquarium, assuming a total pressure of 1.0 atm and a mole fraction for nitrogen of 0.78.
14. Solutions
Henry's Law Calculations
Multiple Choice
At a certain temperature, the solubility of N2 gas in water at 1.75 atm is 41.3 mg of N2 gas per 100 g water. Calculate the solubility of N2 gas in water, at the same temperature, if the partial pressure of N2 gas over the solution is increased to 3.50 atm.
A
41.3 mg of N2 gas per 100 g water
B
82.6 mg of N2 gas per 100 g water
C
123.9 mg of N2 gas per 100 g water
D
20.65 mg of N2 gas per 100 g water
Verified step by step guidance1
Understand that the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid, according to Henry's Law.
Henry's Law can be expressed as: , where is the solubility, is the Henry's Law constant, and is the pressure.
First, calculate the Henry's Law constant using the initial conditions: . Substitute mg/100 g water and atm.
Use the calculated Henry's Law constant to find the new solubility when the pressure is increased to atm: .
Substitute the value of from step 3 into the equation from step 4 to calculate the new solubility of N2 gas in water at atm.
Related Videos
Related Practice
