Answer to Question #165444 in Mechanics | Relativity for Satyam

Question

Explain first law of thermodynamics.

Answer 1

The first law of thermodynamics is the application of the conservation of energy principle to heat and thermodynamic processes: The change in internal energy of a system is equal to the heat added to the system minus the work done by the system.

ΔU=Q - W

The first law makes use of the key concepts of internal energy, heat, and system work. It is used extensively in the discussion of heat engines. The standard unit for all these quantities would be the joule, although they are sometimes expressed in calories or BTU.

It is typical for chemistry texts to write the first law as ΔU=Q+W. It is the same law, of course - the thermodynamic expression of the conservation of energy principle. It is just that W is defined as the work done on the system instead of work done by the system. In the context of physics, the common scenario is one of adding heat to a volume of gas and using the expansion of that gas to do work, as in the pushing down of a piston in an internal combustion engine. In the context of chemical reactions and processes, it may be more common to deal with situations where work is done on the system rather than by it.