Answer :
Final answer:
The partial pressure of oxygen in the air with nitrogen at 82 kPa and CO₂ + H₂O at 0.77 kPa at a total atmospheric pressure of 100 kPa is 17.23 kPa, found by subtracting the partial pressures of nitrogen, carbon dioxide, and water vapor from the total atmospheric pressure.
Explanation:
The partial pressure of oxygen in the air at a total atmospheric pressure of 100 kPa, with nitrogen at 82 kPa and CO₂ + H₂O at 0.77 kPa, can be found using Dalton's Law of Partial Pressures. Dalton's Law states that the total pressure of a mixture of gases is the sum of their individual partial pressures. Therefore, the partial pressure of oxygen (Po₂) can be calculated as:
Po₂ = Patm - (PN₂ + PCO₂ + PH₂O)
Given:
- Patm = 100 kPa
- PN₂ = 82 kPa
- PCO₂ + PH₂O = 0.77 kPa
Substitute these values into the equation:
Po₂ = 100 kPa - (82 kPa + 0.77 kPa)
Po₂ = 100 kPa - 82.77 kPa
Po₂ = 17.23 kPa
Therefore, option b) 17.23 kPa is the correct answer for the partial pressure of oxygen in the air in this scenario.
