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DHDJ

The notes cover fundamental concepts of thermodynamics, including types of systems, laws, and processes. Key laws discussed are the Zeroth, First, and Second Laws of Thermodynamics, along with thermodynamic processes and work done by gases. The document also addresses heat capacity and the efficiency of heat engines, referencing educational materials for further study.

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thaneesh1113
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16 views4 pages

DHDJ

The notes cover fundamental concepts of thermodynamics, including types of systems, laws, and processes. Key laws discussed are the Zeroth, First, and Second Laws of Thermodynamics, along with thermodynamic processes and work done by gases. The document also addresses heat capacity and the efficiency of heat engines, referencing educational materials for further study.

Uploaded by

thaneesh1113
Copyright
© © All Rights Reserved
We take content rights seriously. If you suspect this is your content, claim it here.
Available Formats
Download as PDF, TXT or read online on Scribd
You are on page 1/ 4

Here is the handwritten-style 2-page note for:

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🔥 Thermodynamics – 2-Page Handwritten Notes


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📘 PAGE 1: Laws and Processes


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1. Thermodynamic System

System: part we observe

Surroundings: everything else

Boundary: separates system and surroundings

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2. Types of Systems

Open: matter + energy exchange (e.g. boiling pot)

Closed: only energy exchange

Isolated: no exchange

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3. Zeroth Law of Thermodynamics


If A = B and B = C thermally ⇒ A = C
➤ Basis of thermometer
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4. First Law of Thermodynamics


Energy Conservation:
ΔQ = ΔU + ΔW

Q = Heat supplied

U = Change in internal energy

🧠
W = Work done BY system
Sign convention:
→ Heat IN = +ve
→ Work BY system = +ve

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5. Thermodynamic Processes

Isothermal (T = constant): ΔU = 0 → Q = W

Adiabatic (Q = 0): ΔU = –W

Isochoric (V = constant): W = 0 → Q = ΔU

Isobaric (P = constant): W = PΔV

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📘 PAGE 2: Work, Heat & Second Law


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6. Work Done by a Gas


→ W = ∫ P dV

Area under P–V curve = work

Expansion: W > 0
Compression: W < 0

🧠 Special Case:
Isothermal for ideal gas:
W = nRT ln(V₂/V₁)

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7. Internal Energy (U)

For ideal gas: ΔU = nCᵥΔT

Monoatomic gas: Cᵥ = 3R/2

Diatomic gas: Cᵥ = 5R/2 (without vibration)

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8. Heat Capacity

C = Q / ΔT

Molar heat capacity (C ) = heat for 1 mole per 1K

Relation:
Cₚ – Cᵥ = R

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9. Second Law of Thermodynamics


→ Heat can't spontaneously flow from cold to hot
→ No engine can convert 100% heat to work

🧠 Kelvin-Planck statement: No cyclic engine can convert heat fully to work.


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10. Efficiency of Heat Engines
η = W / Q₁ = (Q₁ – Q₂) / Q₁ = 1 – Q₂/Q₁

Carnot Efficiency:
η = 1 – T₂/T₁ (T in Kelvin)

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📝 References: NCERT Class 11, D.C. Pandey, JEE PYQs


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