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 (Pa)
• \( P_1, P_2, \dots, P_n \) — Partial pressures of individual gases (Pa)

Explanation: The equation simply sums up all the individual pressures that each gas in a mixture would exert if it were alone in the container.

3. Importance of Partial Pressure Calculation

Details: Understanding partial pressures is essential for gas law calculations, respiratory physiology, industrial gas applications, and predicting gas behavior in chemical reactions.

4. Using the Calculator

Tips: Enter partial pressure values separated by commas (e.g., "101325, 25331.25, 5066.25"). All values should be in Pascals (Pa).

5. Frequently Asked Questions (FAQ)

Q1: What units should I use for pressure?
A: The calculator uses Pascals (Pa), but you can convert from other units. 1 atm = 101325 Pa, 1 mmHg ≈ 133.322 Pa.

Q2: Does Dalton's Law apply to reacting gases?
A: No, Dalton's Law only applies to mixtures of non-reacting gases. Chemical reactions between gases can affect partial pressures.

Q3: How does temperature affect partial pressures?
A: While Dalton's Law itself is temperature-independent, the individual partial pressures may change with temperature according to the Ideal Gas Law.

Q4: What's the relationship between partial pressure and mole fraction?
A: Partial pressure equals total pressure multiplied by the mole fraction of that gas (P_i = P_total × X_i).

Q5: Why is Dalton's Law important in breathing?
A: Gas exchange in lungs depends on partial pressure differences of oxygen and carbon dioxide between alveoli and blood.