🔹 Kinetic Theory of Gases – Stage 1 (Page 2)
1️⃣ Molecular Velocities – Components Concept
Molecular motion in a gas is random in all directions. Hence, velocity of a molecule can be resolved into three mutually perpendicular components:
v = (vx, vy, vz)
Due to randomness:
- ⟨vx⟩ = ⟨vy⟩ = ⟨vz⟩ = 0
- ⟨vx2⟩ = ⟨vy2⟩ = ⟨vz2⟩
2️⃣ Mean Square Speed
The average of the square of molecular speeds is called mean square speed.
⟨v2⟩ = ⟨vx2⟩ + ⟨vy2⟩ + ⟨vz2⟩
Since all three components are equal:
⟨v2⟩ = 3⟨vx2⟩
3️⃣ Derivation of Gas Pressure (Key JEE Concept)
Consider a cubical container of side L, containing N molecules, each of mass m.
When a molecule hits the wall perpendicular to x-axis:
- Initial momentum = m vx
- Final momentum = −m vx
- Change in momentum = 2m vx
Time between successive collisions with same wall:
Δt = 2L / vx
Force exerted by one molecule:
F = (2m vx) / (2L / vx) = m vx2 / L
4️⃣ Total Pressure of Gas
Pressure = Total force / Area
P = (Nm / V) ⟨vx2⟩
Using ⟨v2⟩ = 3⟨vx2⟩:
P = (1/3) (Nm / V) ⟨v2⟩
5️⃣ Important Results to Remember
- Pressure is due to molecular collisions
- Only velocity component perpendicular to wall contributes
- Pressure ∝ mean square speed
JEE Exam Notes
- This derivation is frequently tested conceptually
- Know assumptions clearly
- Pressure formula links microscopic & macroscopic physics
✔ Stage 1 – Page 2 COMPLETE
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