Final answer:
Using Henry's Law, the solubility of oxygen at 25 °C increases proportionally with pressure. At 4.0 atm, which is four times the initial pressure, the solubility of oxygen in water is 0.164 g/l, which corresponds to choice 'c' (0.16 g/l).
Step-by-step explanation:
The solubility of oxygen gas in water at a certain temperature and pressure can be calculated using Henry's Law, which states that the solubility of a gas in a liquid is directly proportional to the pressure of that gas above the liquid. Given that the solubility of oxygen at 25 °C and 1.0 atm is 0.041 g/l, we can apply this law to find the solubility at 4.0 atm. According to Henry's Law, if the pressure increases, the solubility will also increase proportionally. Thus, at 4.0 atm (four times the initial pressure), the solubility would be:The solubility of oxygen gas in water at 25 °C and 1.0 atm pressure of oxygen is 0.041 g/l.
To find the solubility of oxygen in water at 4.0 atm and 25 °C, we can use the concept of Henry's Law. According to Henry's Law, the solubility of a gas is directly proportional to its partial pressure.
So, the solubility of oxygen in water at 4.0 atm and 25 °C would be 0.041 g/l, which is option a.