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. More gas molecules are soluble as pressure is increased.
C. The solubility of a gas decreases with a decrease in pressure.
D. The solubility of nitrogen gas at 2.00 atmatm is twice the solubility of the gas at 1.00 atmatm.
E. The concentration of gas particles in the solution is higher at 4.25 atmatm than at 1.00 atmatm.
F. Fewer gas molecules are soluble at higher pressures.
G. As pressure decreases, the concentration of gas molecules in the solution increases.

B, C, D, E

Explanation:

According to Henry's law, as the pressure is increased, the solubility of a given gas increases. So, solubility is directly proportional to pressure.

Thus, the following statements are correct:

B. More gas molecules are soluble as pressure is increased.

Is correct because as the pressure is increased, the solubility increases.

C. The solubility of a gas decreases with a decrease in pressure.

Is correct because solubility and pressure are directly proportional: if the pressure is decreased, the solubility will be decreased.

D. The solubility of nitrogen gas at 2.00 atm is twice the solubility of the gas at 1.00 atm.

Is correct because 2.00 atm is twice 1.00 atm, so if the pressure is increased twice, the solubility is increased twice.

E. The concentration of gas particles in the solution is higher at 4.25 atm than at 1.00 atm.

Is correct because 4.25 atm>1.00 atm (the higher the pressure, the higher the solubility, and therefore the concentration of gas particles in solution).

The remaining options (A, G) are incorrect. They contradict Henry's law.

pv=nrt

explanation: