FIRST LAW OF THERMODYNAMICS

 

First law of the thermodynamics is defined as an application of energy conservation.  The law concentrates on the concept of the internal energy, system work, and the heat.  This law is mostly used to discuss the heat engines. The standard unit to express the quantities used in the first law of thermodynamics is joules though at times are expressed in terms of calories or the BTU.   The total energy of a specified system remains constant. The law states that the energy can either be destroyed or created but it is transformed from one form to another.   First law of thermodynamics is written as ∆U=QW. W stands for work done on the system. Thermodynamics is one of the branches of physics that normally deals with both work and energy.  Helmholtz free energy, the internal energy, and Gibbs free energy are the thermodynamics potentials that are commonly used in the chemical thermodynamics of the reactions and the non-cyclic process. The first full statement of the first law of thermodynamics was set by R. Clausius and W. Rankine.

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