Illustrate the relationship between a pressure of a gas above a liquid and the solubility of the gas in the liquid. Determine the concentration of CO2 in a carbonated beverage bottled under 4.0 atm of CO2. (a) If the mole fraction of CO2 in the air is 0.00355, how many times more concentrated is the CO2 in the unopened bottle than it is in a glass of the beverage that has gone completely flat? (b) Use the kinetic-molecular theory of gases to explain why the solubility of a gas is proportional to its pressure over the liquid.© BrainMass Inc. brainmass.com October 24, 2018, 5:52 pm ad1c9bdddf
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The solubility of a gas in a liquid depends on temperature, the partial pressure of the gas over the liquid, the nature of the solvent and the nature of the gas. The most common solvent is water.
Gas solubility is always limited by the equilibrium between the gas and a saturated solution of the gas. The dissolved gas will always follow Henry's law.
The concentration of dissolved gas depends on the partial pressure of the gas. The partial pressure controls the number of gas molecule collisions with the surface of the solution.
Henry's law states that the ratio of ...
The solution demonstrates how to explain Henry's Law using the kinetic theory of gases.
Finding solubility of a gas using pressure
The solubility of N2 in blood at 37°C and at a partial pressure of 0.80 atm is 5.6 10-4 mol/L. A deep-sea diver breathes compressed air with the partial pressure of N2 equal to 3.6 atm. Assume that the total volume of blood in the body is 5.0 L. Calculate the amount of N2 gas released (in liters at 37°C and 1.1 atm) when the diver returns to the surface of the water, where the partial pressure of N2 is 0.80 atm.
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