🔹 Kinetic Theory of Gases – Stage 1 (Page 3)

1️⃣ Root Mean Square (RMS) Speed

The RMS speed is defined as the square root of the mean of the squares of molecular speeds.

vrms = √⟨v2

From pressure equation:

P = (1/3)(Nm/V)⟨v2

Rearranging:

⟨v2⟩ = 3P / ρ

where ρ = mass density = Nm / V


2️⃣ RMS Speed in Terms of Temperature

Using ideal gas equation:

PV = nRT

For one molecule:

P = (NkT) / V

Substituting into pressure equation:

(1/3) m⟨v2⟩ = kT

Therefore,

vrms = √(3kT / m)

In molar form:

vrms = √(3RT / M)


3️⃣ Translational Kinetic Energy of a Gas Molecule

Average kinetic energy per molecule:

⟨E⟩ = (1/2)m⟨v2

Using ⟨v2⟩ = 3kT / m:

⟨E⟩ = (3/2)kT

Important: Average kinetic energy depends only on temperature, not on mass or nature of gas.


4️⃣ Kinetic Energy per Mole of Gas

For one mole:

E = (3/2)RT

This result is valid for all ideal gases.


5️⃣ Key Comparisons (JEE Favourite)

  • At same temperature: lighter gas → higher RMS speed
  • vrms ∝ √T
  • vrms ∝ 1 / √M

 JEE Exam Notes

  • Kinetic energy depends only on temperature
  • Speed distribution differs, but ⟨E⟩ is same
  • Used heavily in comparative MCQs

✔ Stage 1 – Page 3 COMPLETE

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