Difference between adiabatic and isothermal process

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In the subject thermodynamics, there are two often discussed concepts that are mostly used in many industrial practical applications. These concepts are the adiabatic and isothermal processes. Both of these processes are opposite sides of the coin. Before we start our discussion on the difference between them. First of all, we must know what is the adiabatic process? and what is the isothermal process?

What is the adiabatic process?

A process without transfer of heat or mass between a thermodynamic system and surroundings. An adiabatic process, in which the working substance neither receives nor given out heat or mass to the surroundings, during the expansion or compression is called an adiabatic process.

What is the isothermal process?

The process in which the temperature of the working substance remains constant during its expansion or compression is called isothermal or constant-temperature process.

Difference between adiabatic and isothermal process: 

  • Work done is due to a change in internal energy in the adiabatic process, whereas work done is due to the change in the net heat content in the thermodynamic system in the isothermal process. 
  • The temperature can be varied in the adiabatic process, it is not the case in the isothermal process.  
  • There is no transfer of heat in the adiabatic process, and isothermal process there is a transfer of heat. 
  • The transformation of the adiabatic process is fast, and the transformation of the isothermal process is slow. 
  • The pressure is less at a given volume in the adiabatic process, while it is more at a given volume in the isothermal process.
  • An adiabatic process no heat exchanges so Q = 0 and ΔT ≠ 0 and an isothermal process, ΔT = 0 and therefore ΔU = 0 but Q ≠ 0.
  • An adiabatic process is a non-reversible constant enthalpy process and the isothermal process is a constant temperature process. 

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