🔥 Thermodynamics – Stage 1

Page 8 : Heat Capacity & Mayer’s Relation (JEE Core)

Heat Capacity tells how much heat is required to raise temperature.

1️⃣ Heat Capacity (General Definition)

C = ΔQ / ΔT
• Depends on process
• Depends on constraints (P or V constant)

2️⃣ Heat Capacity at Constant Volume (Cv)

Volume remains constant → No work done
Cv = (ΔQ / ΔT)V
From First Law:
ΔQ = ΔU

Therefore,
Cv = (∂U / ∂T)
⚠ At constant volume → All heat increases internal energy

3️⃣ Heat Capacity at Constant Pressure (Cp)

Pressure remains constant → Work is done
Cp = (ΔQ / ΔT)P
ΔQ = ΔU + PΔV
⚠ Heat supplied increases internal energy + does work

4️⃣ Relation Between Cp and Cv

For all gases:
Cp > Cv
Reason: Extra heat is used to perform work at constant pressure

5️⃣ Mayer’s Relation (Most Important)

Cp − Cv = R
Valid only for ideal gases
R → Universal gas constant

6️⃣ Degrees of Freedom (f)

Energy storage modes of gas molecules
Cv = (f/2)R
Cp = ((f + 2)/2)R
Gas f Cv Cp
Monoatomic 3 3R/2 5R/2
Diatomic 5 5R/2 7R/2
Polyatomic 6 3R 4R

7️⃣ JEE-Trap Notes

⚠ Mayer’s relation fails for real gases
⚠ Cp, Cv are process dependent
⚠ Use degrees of freedom carefully

👉 Next Page:
Page 9 – Adiabatic Process & Poisson’s Equations

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