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Thermodynamics Laws

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Zeroth Law of Thermodynamics

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If two systems are each in thermal equilibrium with a third system, they are in thermal equilibrium with each other. This law provides the basis for the concept of temperature.

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First Law of Thermodynamics

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The total energy of an isolated system is constant; energy can be transformed from one form to another but can be neither created nor destroyed. This law is essentially a statement of the conservation of energy. It can be expressed as

ΔU=QW\Delta U = Q - W
, where ΔU\Delta U is the change in internal energy, QQ is the heat added to the system, and WW is the work done by the system.

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Second Law of Thermodynamics

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In any cyclic process, the entropy will either increase or remain the same. This law predicts the direction of spontaneous processes and indicates that energy has quality as well as quantity. It's often associated with the principle that heat cannot spontaneously transfer from a colder body to a hotter one.

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Third Law of Thermodynamics

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As the temperature of a system approaches absolute zero, the entropy of a perfect crystal approaches a constant minimum. This law implies that it is impossible to reach absolute zero in a finite number of stages. It can be useful in defining the absolute entropy of substances.

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