🔹 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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