🔹 Kinetic Theory of Gases – Stage 1 (Page 9)
1️⃣ Maxwell–Boltzmann Distribution of Speeds
At a given temperature, gas molecules do not have the same speed. Instead, their speeds are distributed according to Maxwell’s distribution law.
The number of molecules having speed between v and v + dv is given by:
dN ∝ v² e−mv²/2kT dv
2️⃣ Maxwell Speed Distribution Curve
- Y-axis → Number of molecules
- X-axis → Speed (v)
- Curve starts from origin
- Rises to a maximum and then falls asymptotically
Area under the curve = Total number of molecules
3️⃣ Characteristic Speeds of Gas Molecules
| Speed | Expression |
|---|---|
| Most Probable Speed (vmp) | √(2RT / M) |
| Average Speed (vavg) | √(8RT / πM) |
| Root Mean Square Speed (vrms) | √(3RT / M) |
4️⃣ Relation Between Speeds
vmp < vavg < vrms
Ratio:
vmp : vavg : vrms = √2 : √(8/π) : √3
5️⃣ Effect of Temperature on Distribution
- Increase in temperature → curve flattens
- Peak shifts towards higher speed
- Area under curve remains constant
6️⃣ Effect of Molecular Mass
- Lighter gas → higher speeds
- Heavier gas → lower speeds
- At same temperature, all gases have same average kinetic energy
⟨KE⟩ = (3/2)kT
7️⃣ Important Graph-Based Results
- Area under curve does NOT depend on temperature
- Higher T → broader curve
- For same T, lighter gas curve shifts right
8️⃣ JEE Advanced Tricks
- Speeds ∝ √T
- Speeds ∝ 1 / √M
- Ratio questions are faster than absolute calculations
- Always compare rms speeds in energy-based questions
9️⃣ Common JEE Traps
- Confusing vavg with vrms
- Assuming all molecules have same speed
- Wrong interpretation of graph area
✔ Stage 1 – Page 9 COMPLETE
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