🔹 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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