1. What is Partial Pressure?

Partial pressure is the pressure that a gas in a mixture would exert if it occupied the entire volume alone at the same temperature. It's a way to express the contribution of each gas to the total pressure of a gas mixture.

2. Dalton's Law of Partial Pressures

The calculator uses Dalton's Law:

Where:

• \( P_i \) — Partial pressure of the gas (atm)
• \( n_i \) — Moles of the gas (mol)
• \( n_{total} \) — Total moles of all gases (mol)
• \( P_{total} \) — Total pressure of the gas mixture (atm)

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

3. Importance of Partial Pressure

Details: Partial pressure is crucial in gas laws, respiratory physiology (oxygen and carbon dioxide exchange), industrial gas applications, and chemical equilibrium calculations.

4. Using the Calculator

Tips: Enter the moles of the gas, total moles of all gases, and total pressure. All values must be positive numbers. The calculator will determine the partial pressure of the specified gas.

5. Frequently Asked Questions (FAQ)

Q1: What units should I use?
A: The calculator uses moles (mol) for quantity and atmospheres (atm) for pressure. Convert your values to these units before calculation.

Q2: Does this work for ideal gases only?
A: Dalton's Law applies exactly to ideal gases and is a good approximation for real gases at low pressures and high temperatures.

Q3: Can I calculate mole fraction from partial pressure?
A: Yes, mole fraction equals partial pressure divided by total pressure (X_i = P_i/P_total).

Q4: How does temperature affect partial pressure?
A: At constant volume, increasing temperature increases both partial and total pressures proportionally.

Q5: Is this applicable to liquid solutions?
A: While similar concepts exist for solutions, this calculator specifically deals with gas mixtures.