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. This principle is important in understanding gas diffusion and separation processes.

2. How Does the Calculator Work?

The calculator uses Graham's Law equation:

Where:

• \( Rate \) — Effusion rate (relative units)
• \( M \) — Molar mass of the gas (g/mol)

Explanation: The equation shows that lighter gases effuse faster than heavier ones. For example, hydrogen (M = 2 g/mol) effuses much faster than oxygen (M = 32 g/mol).

3. Importance of Effusion Rate

Details: Understanding effusion rates is crucial in chemical engineering, gas separation technologies, and predicting gas behavior in different environments.

4. Using the Calculator

Tips: Enter the molar mass of the gas in g/mol. The value must be greater than 0. The calculator will output the relative effusion rate.

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. Both follow similar principles but differ in their mechanisms.

Q2: How do I compare effusion rates of two gases?
A: The ratio of effusion rates is equal to the inverse ratio of the square roots of their molar masses: \( \frac{r_1}{r_2} = \sqrt{\frac{M_2}{M_1}} \).

Q3: What are typical molar mass values?
A: Common gases range from 2 g/mol (H₂) to 44 g/mol (CO₂). Air averages about 29 g/mol.

Q4: Does temperature affect effusion rate?
A: While Graham's Law focuses on molar mass, temperature does affect absolute effusion rates (higher temperature = faster effusion).

Q5: What practical applications use this principle?
A: Gas separation processes, leak detection, and isotope separation (like uranium enrichment) all utilize Graham's Law principles.