Final answer:
The total pressure of the air mixture, which includes partial pressures of oxygen, nitrogen, carbon dioxide, and water vapor, is the sum of their individual pressures, amounting to 672 mmHg.
Step-by-step explanation:
The total pressure of a gas mixture is the sum of the partial pressures of the individual gases within the mixture. Based on the given pressures, oxygen is at 70 mmHg, nitrogen at 548 mmHg, carbon dioxide at 23 mmHg, and water vapor at 31 mmHg. To find the total pressure of the sample, we simply add these values together:
- Oxygen (O₂): 70 mmHg
- Nitrogen (N₂): 548 mmHg
- Carbon Dioxide (CO₂): 23 mmHg
- Water Vapor (H₂O): 31 mmHg
The calculation would be: 70 mmHg + 548 mmHg + 23 mmHg + 31 mmHg = 672 mmHg.
Therefore, the total pressure of the air mixture is 672 mmHg.