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

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

2. How Does the Calculator Work?

The calculator uses Dalton's Law equation:

Where:

• \( P_i \) — Partial pressure of the gas (Pa)
• \( X_i \) — Mole fraction of the gas (unitless)
• \( P_{total} \) — Total pressure of the gas mixture (Pa)

Explanation: The partial pressure of a gas in a mixture is equal to the mole fraction of that gas multiplied by the total pressure of the mixture.

3. Importance of Partial Pressure Calculation

Details: Partial pressure calculations are crucial in respiratory physiology, gas exchange processes, chemical reactions involving gases, and industrial gas applications.

4. Using the Calculator

Tips: Enter mole fraction (between 0 and 1) and total pressure in Pascals (Pa). Both values must be valid (mole fraction between 0-1, total pressure > 0).

5. Frequently Asked Questions (FAQ)

Q1: What is mole fraction?
A: Mole fraction is the ratio of the number of moles of a component to the total number of moles in the mixture.

Q2: Can Dalton's Law be applied to liquids?
A: No, Dalton's Law specifically applies to mixtures of non-reacting gases.

Q3: What are common units for partial pressure?
A: While we use Pascals (Pa) here, other common units include atmospheres (atm), mmHg, and torr.

Q4: Does temperature affect partial pressure?
A: Temperature affects the total pressure of the gas mixture, which in turn affects partial pressures, but the mole fractions remain constant.

Q5: How is this used in real-world applications?
A: Applications include scuba diving (gas mixtures), medical oxygen therapy, industrial gas processes, and atmospheric science.