Final answer:
The partial pressure of oxygen can be calculated using Dalton's law of partial pressures. In this case, the partial pressure of oxygen is 743.2 torr.
Step-by-step explanation:
The partial pressure of oxygen can be calculated using Dalton's law of partial pressures. According to Dalton's law, the total pressure of the gas mixture is equal to the sum of the partial pressures of each gas component. In this case, the total pressure is 763.0 torr. Subtracting the vapor pressure of water at 22.3 degrees Celsius, which is 19.8 torr, from the total pressure will give us the partial pressure of the oxygen:
Oxygen partial pressure = Total pressure - Vapor pressure of water
Oxygen partial pressure = 763.0 torr - 19.8 torr = 743.2 torr