1. What is Partial Pressure of Oxygen?

The partial pressure of oxygen (P_O2) is the pressure that oxygen would exert if it alone occupied the volume of the mixture at the same temperature. It's a fundamental concept in gas mixtures and respiratory physiology.

2. How Does the Calculator Work?

The calculator uses Dalton's Law of Partial Pressures:

Where:

• \( P_{O_2} \) — Partial pressure of oxygen (atm)
• \( Moles_{O_2} \) — Moles of oxygen in the mixture (mol)
• \( Total\ Moles \) — Total moles of all gases in the mixture (mol)
• \( P_{total} \) — Total pressure of the gas mixture (atm)

Explanation: The partial pressure of a gas is proportional to its mole fraction in the gas mixture.

3. Importance of Partial Pressure Calculation

Details: Partial pressure calculations are essential in respiratory physiology, diving medicine, anesthesia, and industrial gas applications. It determines gas exchange in lungs and tissues.

4. Using the Calculator

Tips: Enter moles of oxygen, total moles of gas, and total pressure. All values must be positive numbers. The result is given in atmospheres (atm).

5. Frequently Asked Questions (FAQ)

Q1: What is normal P_O2 in arterial blood?
A: Normal arterial P_O2 is about 75-100 mmHg (0.099-0.132 atm) at sea level.

Q2: How does altitude affect P_O2?
A: As altitude increases, total atmospheric pressure decreases, reducing P_O2 in inspired air.

Q3: What's the difference between P_O2 and oxygen concentration?
A: P_O2 measures the pressure exerted by oxygen, while concentration measures the amount per volume. P_O2 determines diffusion rates.

Q4: How is this used in diving?
A: Divers calculate P_O2 at depth to avoid oxygen toxicity (typically limited to 1.4-1.6 atm).

Q5: What units are used for P_O2?
A: Common units include atm, mmHg, and kPa. This calculator uses atm (1 atm = 760 mmHg = 101.325 kPa).