Thermodynamics Flashcards

Grade 11 · Science · Flashcards

Essential thermodynamics vocabulary, laws, and formulas for Grade 11 advanced physics.

Flashcards

First Law of Thermodynamics

ΔU = Q - W; energy is conserved — internal energy change equals heat added minus work done by the system.

Second Law of Thermodynamics

Entropy of an isolated system always increases or stays constant; heat flows spontaneously from hot to cold.

Carnot Efficiency Formula

η = 1 - (T_cold/T_hot); temperatures must be in Kelvin; represents the absolute maximum efficiency of any heat engine.

Entropy

Measure of disorder in a system; ΔS = Q_rev/T for reversible processes; always increases in irreversible processes.

Adiabatic Process

Q = 0; no heat exchange. Work done on/by gas changes internal energy: ΔU = -W.

Isothermal Process

Constant temperature (ΔT = 0); for ideal gas ΔU = 0, so all heat input equals work output: Q = W.

Isobaric Process

Constant pressure; work done W = PΔV; heat added changes both internal energy and does work.

Isochoric Process

Constant volume; W = 0; all heat added goes entirely into changing internal energy: ΔU = Q.

Specific Heat Capacity (c)

Amount of heat per unit mass per degree of temperature change; Q = mcΔT.

Latent Heat (L)

Heat absorbed or released per unit mass during a phase change at constant temperature; Q = mL.

Heat Engine

Converts thermal energy to mechanical work by operating between hot (T_H) and cold (T_C) reservoirs; W = Q_H - Q_C.

Thermal Equilibrium

State where two objects in contact have reached the same temperature and no net heat flows between them.

Absolute Zero

0 K (−273.15°C); the lowest possible temperature where molecular motion theoretically ceases; entropy of perfect crystal = 0.

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