1. What is Graham's Law of Effusion?

Graham's Law states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass. Effusion is the process by which gas molecules pass through a tiny opening from one container to another.

2. How Does the Calculator Work?

The calculator uses Graham's Law equation:

Where:

• \( \text{Rate}_1 \) — Effusion rate of gas 1 (unitless)
• \( \text{Rate}_2 \) — Effusion rate of gas 2 (unitless)
• \( \text{MW}_1 \) — Molecular weight of gas 1 (g/mol)
• \( \text{MW}_2 \) — Molecular weight of gas 2 (g/mol)

Explanation: Lighter gases effuse faster than heavier ones. The rate ratio depends on the inverse square root of their molecular weights.

3. Applications of Effusion Rates

Details: This principle is used in gas separation techniques, determining molecular weights of gases, and explaining real-world phenomena like helium balloon deflation.

4. Using the Calculator

Tips: Enter molecular weights of both gases. You can optionally enter one rate to calculate the other, or leave both blank to just see the ratio.

5. Frequently Asked Questions (FAQ)

Q1: What's the difference between effusion and diffusion?
A: Effusion is gas escaping through a tiny hole, while diffusion is gas spreading out in space.

Q2: Does temperature affect effusion rates?
A: Yes, but the ratio between two gases' rates at the same temperature depends only on their molecular weights.

Q3: What are some common examples of effusion?
A: Helium leaking from balloons faster than air, uranium isotope separation, and gas separation in industrial processes.

Q4: Why is the ratio unitless?
A: The equation compares relative rates, so the units cancel out. Absolute rates would have units (e.g., mol/s).

Q5: Can this be used for gas mixtures?
A: Yes, but each component gas would effuse at its own rate based on its molecular weight.