Adiabatic Process.

                               

        ADIABATIC PROCESS.

When there is no heat transfer between the system and its surroundings, a thermodynamic process known as an adiabatic process occurs. As a result, because the system is thermally isolated, there is no heat energy transfer between it and its surroundings during an adiabatic process. Any change in the internal energy of the system during such a process is solely the result of work done on or by the system. This work can be accomplished through a variety of mechanisms, such as gas compression or expansion, or changes in the internal energy of a system caused by physical or chemical reactions. For example, when a gas is compressed adiabatically, the environment exerts force on the gas, increasing its pressure and temperature. When a gas expands adiabatically, the pressure and temperature fall because the gas exerts force on the environment.

The adiabatic process is described by the first law of thermodynamics, which states that the internal energy change of a system is equal to the work done on or by the system. A common mathematical expression for this relationship is dU = -pdV, where dU is the change in internal energy, p is the change in pressure, and dV is the change in system volume.

                       Adiabatic Compression.

This is a process in which no heat enters or exits the system (Q = 0). However, the gas can be compressed by applying external force or expanded by utilizing its internal energy. As a result, an adiabatic process may cause changes in the system's pressure, volume, and temperature. For an adiabatic process, the first law changes to U = W. This implies that either the gas does the work at the expense of internal energy or the system does the work at the expense of internal energy.

                  Adiabatic Expansion.

                      references

Perrot, P. (1998). A to Z of Thermodynamics. Oxford University Press on Demand.