Kinetic Theory of Gases Cheatsheet

Cheat Codes & Shortcuts

• Definition: Explains macroscopic gas properties via microscopic particle motion.
• Ideal Gas Law: \( PV = nRT \)
• Pressure: \( P = \frac{1}{3} \frac{N}{V} m \langle v^2 \rangle \)
• Mean Free Path: \( \lambda = \frac{1}{\sqrt{2} \pi d^2 \frac{N}{V}} \)
• Kinetic Energy: Average KE per molecule \( \langle KE \rangle = \frac{3}{2} k T \)
• RMS Speed: \( v_{rms} = \sqrt{\frac{3RT}{M}} \)
• Maxwell-Boltzmann Distribution: Describes speed distribution of gas molecules.
• Degrees of Freedom: \( f = 3 \) (monatomic), \( f = 5 \) (diatomic at moderate T).
• Equipartition Theorem: Each degree of freedom contributes \( \frac{1}{2} k T \).
• Boltzmann Constant: \( k = \frac{R}{N_A} \approx 1.38 \times 10^{-23} \, \text{J/K} \).

Quick Reference Table

Advice

Kinetic Theory of Gases Quick Tips

• Ideal Gas Law: Use \( PV = nRT \) to relate macroscopic properties.
• RMS Speed: Calculate \( v_{rms} = \sqrt{\frac{3RT}{M}} \) for molecular speed.
• Kinetic Energy: Relate temperature to \( \langle KE \rangle = \frac{3}{2} k T \).
• Mean Free Path: Use \( \lambda \) to estimate collision frequency.
• Maxwell-Boltzmann: Understand speed distribution for real gases.