Which of the following statements correctly explain the relationship between the solubility of a gas and its pressure? a. As pressure is increased, the rate at which gas molecules enter the solution decreases. b. As pressure decreases, the concentration of gas molecules in the solution increases. c. The solubility of a gas decreases with a decrease in pressure. d. More gas molecules are soluble as pressure is increased. e. The solubility of nitrogen gas at 2.00 atm is twice the solubility of the gas at 1.00 atm. f. The concentration of gas particles in the solution is higher at 4.25 atm than at 1.00 atm. g. Fewer gas molecules are soluble at higher pressures.

Question

Chemistry

Carlson

5 November, 12:49

Which of the following statements correctly explain the relationship between the solubility of a gas and its pressure? a. As pressure is increased, the rate at which gas molecules enter the solution decreases. b. As pressure decreases, the concentration of gas molecules in the solution increases. c. The solubility of a gas decreases with a decrease in pressure. d. More gas molecules are soluble as pressure is increased. e. The solubility of nitrogen gas at 2.00 atm is twice the solubility of the gas at 1.00 atm. f. The concentration of gas particles in the solution is higher at 4.25 atm than at 1.00 atm. g. Fewer gas molecules are soluble at higher pressures.

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Answers (1)

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Abel Ashley · Answer 1

d. More gas molecules are soluble as pressure is increased

Explanation:

Liquids and solids exhibit practically no change of solubility with changes in pressure. Gases as might be expected, increase in solubility with an increase in pressure.

Henry's Law states that: The solubility of a gas in a liquid is directly proportional to the pressure of that gas above the surface of the solution.

If the pressure is increased, the gas molecules are "forced" into the

solution since this will best relieve the pressure that has been applied and as a result The number of gas molecules dissolved in solution will be increased