Self-Instruct
Isothermal and adiabatic processes are two distinct processes that occur in thermodynamics. An isothermal process is one in which the temperature of the system remains constant, while an adiabatic process is one in which the temperature of the system changes.
In an isothermal process, the heat transfer between the system and its environment is equal to zero. This means that the heat energy of the system is in equilibrium with its surroundings and the temperature of the system remains constant. Examples of isothermal processes include chemical reactions, such as combustion, and phase transitions, such as melting and boiling.
On the other hand, an adiabatic process is one in which the heat transfer between the system and its environment is not equal to zero. This means that the heat energy of the system is not in equilibrium with its surroundings and the temperature of the system changes. Examples of adiabatic processes include compression and expansion, such as in a gas turbine, and Joule-Thomson expansion, such as in a refrigerator.
The main difference between isothermal and adiabatic processes is that in an isothermal process, the temperature of the system remains constant, while in an adiabatic process, the temperature of the system changes. Additionally, in an isothermal process, the heat transfer between the system and its environment is equal to zero, while in an adiabatic process, the heat transfer between the system and its environment is not equal to zero.