1. What is Dalton's Law of Partial Pressures?

Dalton's Law states that in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of the individual gases. This fundamental principle is crucial in gas chemistry and physics.

2. How Does the Calculator Work?

The calculator uses Dalton's Law equation:

Where:

• \( P_{total} \) — Total pressure of the gas mixture
• \( P_1, P_2, \ldots, P_n \) — Partial pressures of individual gases

Explanation: Each gas in a mixture exerts pressure independently, and the total pressure is simply the sum of all these individual pressures.

3. Importance of Dalton's Law

Details: Dalton's Law is essential for understanding gas behavior in mixtures, calculating gas concentrations, and solving problems in respiratory physiology, atmospheric science, and industrial gas processes.

4. Using the Calculator

Tips: Enter partial pressures separated by commas (e.g., "1.2, 0.8, 3.5"). All values should be in the same units (typically atm). The calculator will sum all valid numbers entered.

5. Frequently Asked Questions (FAQ)

Q1: What are partial pressures?
A: The pressure that each gas in a mixture would exert if it alone occupied the entire volume at the same temperature.

Q2: Does Dalton's Law apply to reacting gases?
A: No, it only applies to non-reacting gas mixtures. Chemical reactions can change the number of gas molecules and thus the pressures.

Q3: What units should be used?
A: Any pressure unit can be used (atm, mmHg, kPa, etc.) as long as all values are in the same unit.

Q4: How does temperature affect partial pressures?
A: Temperature affects all gas pressures equally (via the Ideal Gas Law), so the proportion of partial pressures remains constant at constant volume.

Q5: What's the relationship with mole fraction?
A: Partial pressure equals total pressure multiplied by mole fraction (\( P_i = X_i \times P_{total} \)).