First law of thermodynamics
For a closed thermodynamic system, the first law of thermodynamics may be stated as: δ Q = d U + δ W {\displaystyle \delta Q=\mathrm {d} U+\delta W} , or equivalently, d U = δ Q − δ W , {\displaystyle \mathrm {d} U=\delta Q-\delta W,} where δ Q {\displaystyle \delta Q} is the quantity of energy added to the system by a heating process, δ W {\displaystyle \delta W} is the quantity of energy lost by the system due to work done by the system on its surroundings and d U {\displaystyle \mathrm {d} U} is the change in the internal energy of the system. The δ's before the heat and work terms are used to indicate that they describe an increment of energy which is to be interpreted somewhat differently than the d U {\displaystyle \mathrm {d} U} increment of internal energy (see Inexact differential). Work and heat refer to kinds of process which add or subtract energy to or from a system, while the internal energ...
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