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Thermal Engineering

Laws of Thermodynamics

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First Law of Thermodynamics

Energy cannot be created or destroyed in an isolated system, only transformed. Stated mathematically, the change in internal energy of a system is equal to the heat added to the system minus the work done by the system:

\Delta U = Q - W

. This law is a statement of the conservation of energy.

Third Law of Thermodynamics

As the temperature of a system approaches absolute zero, the entropy of a perfect crystal approaches a constant minimum. This implies that it's impossible to reach absolute zero in a finite number of steps. Mathematically, for a perfect crystal at absolute zero, $S = 0$ .

Zeroth Law of Thermodynamics

If two systems are each in thermal equilibrium with a third system, then they are in thermal equilibrium with each other. The implication is the establishment of temperature as a fundamental and measurable property of matter.

Second Law of Thermodynamics

The total entropy of a closed system can never decrease over time. It implies that systems will naturally progress towards thermodynamic equilibrium, the state with maximum entropy. One formulation is through the Clausius statement: 'It is impossible for a process to transfer heat from a cooler to a hotter body without any work input'.

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