This chapter covers the fundamental laws of thermodynamics, focusing on heat, work, and energy transfer in systems.
Thermodynamics - Quick Look Revision Guide
Your 1-page summary of the most exam-relevant takeaways from Physics Part - II.
This compact guide covers 20 must-know concepts from Thermodynamics aligned with Class 11 preparation for Physics. Ideal for last-minute revision or daily review.
Complete study summary
Essential formulas, key terms, and important concepts for quick reference and revision.
Key Points
Zeroth Law of Thermodynamics.
Two systems in thermal equilibrium with a third are in equilibrium with each other.
Internal Energy (U).
Sum of kinetic and potential energies of molecules; depends on the state's variables.
Heat vs. Work.
Heat is energy in transit due to temperature difference; work is energy transfer via force.
First Law of Thermodynamics.
∆Q = ∆U + ∆W; energy conservation principle applied to heat and work.
Specific Heat Capacity.
Amount of heat needed to change temperature; defined as s = ∆Q/(m∆T).
Molar Specific Heat Capacity.
Defined as C = ∆Q/(µ∆T); where µ is the number of moles.
Quasi-static Process.
An infinitely slow process ensuring the system is in equilibrium with surroundings.
Isothermal Process.
Occurs at constant temperature; described by PV = constant (Boyle's Law).
Adiabatic Process.
No heat exchange; for an ideal gas, PV^γ = constant, γ = Cp/Cv.
Isochoric Process.
Volume remains constant; no work done; heat changes internal energy.
Isobaric Process.
Pressure remains constant; work done W = P(V2 - V1).
Cyclic Process.
System returns to initial state; ∆U = 0; total heat equals work done.
Second Law of Thermodynamics.
Does not allow 100% efficiency for heat engines; introduces irreversibility.
Kelvin-Planck Statement.
No process converts heat completely into work from a single reservoir.
Clausius Statement.
No process transfers heat from colder to hotter objects without work input.
Reversible Process.
Can return both system and surroundings to original states without external effects.
Carnot Engine Efficiency.
η = 1 - (T2/T1); maximizes efficiency between two temperatures.
Ideal Gas Law.
PV = µRT; relates pressure, volume, temperature, and moles of gas.
Work Done in Isothermal Expansion.
W = µRT ln(V2/V1); work during gas expansion at constant temperature.
Energy Transfer in Adiabatic Process.
Work done alters internal energy, leading to temperature change.
Heat Capacity Relationships.
Cp - Cv = R for ideal gases; specific heats at constant pressure and volume.
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