Final answer:
By applying Henry's Law, we find that the solubility of O₂ in water at 4.00 atm is 2.80 g per liter of water, because the solubility increases proportionally with pressure.
Step-by-step explanation:
The student's question involves the application of Henry’s Law, which states that the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid. In the given problem, at 0 °C and 1.00 atm, 0.70 g of O₂ can dissolve in 1 L of water.
According to Henry's law, if the pressure is increased to 4.00 atm (which is four times the initial pressure), the solubility will also increase fourfold, assuming the temperature remains constant at 0 °C. Therefore, to find the new solubility of O₂ in water at 4.00 atm, you simply multiply the original solubility by 4:
0.70 g × 4 = 2.80 g, Thus, at 0 °C and 4.00 atm, as much as 2.80 g of O₂ can dissolve in 1 L of water.