Rate of Effusion Calculator
Calculate gas effusion and diffusion rates using Graham's law of diffusion
Calculate Rate of Effusion
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Graham's Law Results
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Common Gas Examples
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Graham's Law
Basic Formula
rate₁ / rate₂ = √(M₂ / M₁)
Rate is inversely proportional to square root of molar mass
Key Principle
Lighter gases diffuse and effuse faster than heavier gases
Applications
- • Gas separation processes
- • Isotope enrichment
- • Molecular weight determination
- • Gas leak detection
Diffusion vs Effusion
Diffusion
Gases spread from high to low concentration areas through intermolecular collisions
Effusion
Gas molecules escape through tiny openings without collisions
Speed Rankings
Understanding Graham's Law of Diffusion
What is Graham's Law?
Graham's law states that the rate of diffusion or effusion of a gas is inversely proportional to the square root of its molar mass. This fundamental principle explains why lighter gases move faster than heavier ones under the same conditions.
Historical Background
Formulated by Scottish chemist Thomas Graham in 1846, this law revolutionized our understanding of gas behavior and became crucial for industrial applications like isotope separation.
Mathematical Foundation
- •Based on kinetic molecular theory
- •Assumes ideal gas behavior
- •Equal kinetic energies at same temperature
- •Inverse relationship with molecular mass
Derivation from Kinetic Theory
½m₁v₁² = ½m₂v₂² (Equal kinetic energies)
v₁/v₂ = √(m₂/m₁) (Velocity ratio)
rate₁/rate₂ = √(M₂/M₁) (Rate ratio)
Real-World Applications
- Uranium Enrichment: Separating U-235 from U-238
- Gas Chromatography: Analytical separation techniques
- Natural Gas Processing: Helium separation
- Medical Applications: Anesthetic gas behavior
- Environmental Science: Gas leak detection
Important: Graham's law assumes ideal conditions. Real gases may deviate at high pressures or low temperatures.
Industrial Applications
Isotope Separation
Used in nuclear fuel processing to separate uranium isotopes based on their mass differences.
Gas Purification
Industrial separation of gas mixtures by exploiting different diffusion rates.
Analytical Chemistry
Determining molecular weights of unknown gases through comparative effusion studies.