Solubility of Gas in Liquids — MCQ Practice

The Henry's Law constant for oxygen dissolved in water at $298,\text{K}$ is $K_H = 34.86,\text{kBar}$. If the partial pressure of oxygen in the air is $0.21,\text{atm}$, what is the mole fraction of oxygen dissolved in water at $298,\text{K}$?

Which of the following statements is INCORRECT regarding the solubility of gases in liquids?

The partial pressure of ethane over a saturated solution containing $6.56 \times 10^{-2},\text{g}$ of ethane is $1,\text{bar}$. If the solution contains $5.00 \times 10^{-2},\text{g}$ of ethane, then what will be the partial pressure of the gas (in bar) if the temperature remains the same?

Why do aquatic species prefer colder water?

Which of the following gases would have the highest Henry's Law constant ($K_H$) in water at a given temperature?

A diver is at a depth where the partial pressure of nitrogen gas in his blood is $1.5,\text{atm}$. If the Henry's Law constant for nitrogen in blood at body temperature is $K_H = 6.5 \times 10^4,\text{atm}$, what is the mole fraction of nitrogen dissolved in his blood?