🔹 Kinetic Theory of Gases – Stage 1 (Page 4)
1️⃣ Three Important Molecular Speeds
In a gas, molecules do not move with the same speed. Instead, their speeds are distributed over a range.
The three important speeds are:
- Most Probable Speed (vmp)
- Average Speed (vavg)
- Root Mean Square Speed (vrms)
2️⃣ Most Probable Speed (vmp)
The speed possessed by the maximum number of molecules at a given temperature.
vmp = √(2kT / m)
In molar form:
vmp = √(2RT / M)
3️⃣ Average Speed (vavg)
Arithmetic mean of the speeds of all molecules.
vavg = √(8kT / πm)
In molar form:
vavg = √(8RT / πM)
4️⃣ RMS Speed (vrms)
Defined as the square root of the mean of the squares of speeds.
vrms = √(3kT / m)
In molar form:
vrms = √(3RT / M)
5️⃣ Relation Between Speeds (VERY IMPORTANT)
vmp : vavg : vrms = √2 : √(8/π) : √3
Numerically:
vmp < vavg < vrms
6️⃣ Maxwell–Boltzmann Speed Distribution
The Maxwell distribution curve shows how molecular speeds are distributed at a given temperature.
- Curve is asymmetric
- Peak corresponds to vmp
- Area under curve = total molecules
Effect of temperature:
- Increase in T → curve flattens
- Peak shifts to right
- More high-speed molecules
7️⃣ JEE Exam Traps
- Speeds depend on √T, not T
- At same T, lighter gas moves faster
- KE depends on T, speed depends on mass
- Never confuse speed with kinetic energy
✔ Stage 1 – Page 4 COMPLETE
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