What are the differences between the adiabatic process and i

What are the differences between the adiabatic process and isothermal process? Provide examples.

Solution

In the realm of Physics, specifically in the subject thermodynamics, there are two often discussed concepts that are frequently used in industrial practical application. These concepts are the adiabatic and isothermal processes.

These two processes are the opposite sides of the coin. They are the poles located at opposite ends so to speak. Firstly, otherwise known as an isocaloric process, the adiabatic process is when there’s no transfer of heat from or towards the fluid being worked on. Besides, adiabatic would mean impassable if defined literally. Thus, heat is not able to penetrate.

When there’s an actual gain or heat loss in the surroundings then the process is termed adiabatic. Because the temperature can change in an adiabatic process due to internal system variations, the gas in the system may tend to cool down when expanding. In this connection, it would also mean that its pressure is significantly lesser compared to the other process (isothermal) at a given volume.

As mentioned, the process at the other extreme end that permits transfer of heat to the surroundings, and thus, making the overall temperature constant (do not change) is called an isothermal process. If you come to think of it, the word isothermal when interpreted literally would mean ‘iso’ (the same), ‘thermal’ (temperature). Hence, there is the same temperature.

In a thermodynamic system, the two main processes involved are adiabatic or isothermal. It is regarded as the former when the transformation (fluctuations or variations in temperature) are fast enough that no heat was significantly transferred between the outside environment and the system. When the transformation is very slow in that same system then the process is isothermal because the temperature of the system remains the same through the exchange of heat with the outer environment.