The isothermal and adiabatic processes are used in thermodynamics to explain the behavior of a thermodynamic process and its relationship to temperature variations. To comprehend its actual industrial use, the distinction between isothermal and adiabatic reactions must be grasped. Both of these processes are mentioned more often in thermodynamics. Both of these processes are opposed.
Adiabatic vs Isothermal
The major distinction between adiabatic and isothermal processes is that adiabatic processes take place at different temperatures whereas isothermal processes take place at a constant temperature. The most significant difference between the two parts of the process is that the adiabatic process does not include heat transport to or from the liquid. On either hand, in the isothermal process, heat is transferred to the environment to maintain a constant temperature.
The adiabatic process happens when there is no heat transfer between such a system and its environment. To avoid unwanted heat transmission, the system’s temperature should be adjusted. This adiabatic process may be reversible or irreversible.
An isothermal process occurs at a fixed temperature, but other system parameters can be altered as needed. It is a thermodynamics phenomenon in which the temperatures of a system do not change over time. To maintain thermal equilibrium, heat is transferred into and out of the system at a relatively slow rate. The isothermal Process is the change of a material, item, or even a system at a constant temperature.
Comparison Table Between Adiabatic and Isothermal Process
|PARAMETERS||ADIABATIC PROCESS||ISOTHERMAL PROCESS|
|Pressure||At a given volume, the pressure is lower.||At a given volume, the pressure is higher.|
|Heat Transfer||Heat transfer doesn’t take place.||Heat transfer takes place.|
|Temperature||The internal system variations cause temperature changes.||The temperature remains constant.|
|Enthalpy||Enthalpy changes within the process.||Enthalpy remains constant.|
|Example||Gas expanding in a vacuum container.||Formation of ice from water.|
What is Adiabatic?
An adiabatic process is a thermodynamic process that occurs when there is no heat transfer between a system and its surroundings. Neither heat nor energy is transported into or out of the system in this case. As a result, the only method for energy to be transferred between a body and its environment in an adiabatic process is through effort. It might be either irreversible or reversible.
The settings of a piston, such as with a piston in a gasoline engine, is an instance when adiabatic processes are relevant. The gas shall contract as the piston’s pressure rises. Decompression causes the gas to expand again, causing the piston to move. Adiabatic mechanisms are in charge of this.
Adiabatic expansion is the idealized behavior of a system in which the temperature continues to rise but the pressure remains constant. It refers to a sealed system in general.
The higher internal energy of the airflow in the system equals the exterior work done. The heat from the surrounding atmosphere is not eliminated or added to the system air in this case. The operating pressure tends to be greater than the volume as the temperature rises.
By doing the operation fast, an adiabatic process may be maintained. For instance, if we compress a gas fast in cylinders, the system will not have enough time to transmit thermal energy to the surroundings. The work performed by the system modifies the inner energy of the system in adiabatic processes.
What is Isothermal?
An isothermal process is one in which despite changes in pressure and volume the temperature stays constant. Boyle’s gas law in thermodynamics connects pressure, temperature, and volume. If one remains unchanged, the others will alter in proportion to it. Whenever the pressure and volume of the gas are inversely proportional, the temperature of a gas remains constant.
To maintain the system’s temperature constant, heat must be moved into or relocated out of the system.
For example, when a material, like water, reaches its melting or boiling point, the pressure and temperature stay constant despite changes in phase, volume, and heat energy.
The Carnot engine is an important manufacturing utilization of the isothermal process. To keep the system’s temperature stable, work should be done here on systems or by the systems in the environment; working on the gases increases energy, which raises the temperature.
However, if indeed the temperature increases over the setpoint, the system begins to function on the environment. When the temperature of the system drops, however, the energy is released as heat into the environment.
Main Difference Between Adiabatic and Isothermal
- In an adiabatic system, the temperatures of a gas decrease as it expands, whereas in an isothermal system, the temperature remains constant as the gas expands.
- In an adiabatic system, pressure is inversely proportional to volume, whereas pressure in an isothermal system is inversely proportional to volume.
- In an adiabatic system, heat does not vary, but it does in an isothermal system.
- In an adiabatic process, internal energy changes, causing expansion, but in an isothermal process, expansion occurs by absorption of heat from the environment.
- An adiabatic process system is thermally separated from its surroundings and hence requires an isolated system, whereas an isothermal process system is not thermally insulated from its surroundings and thus requires an open or closed system.
- The work done in an adiabatic process is due to changes in internal energy whereas the work done in an isothermal process is due to the system’s net heat content.
- An adiabatic system compresses by adding heat to the system’s internal energy, whilst an isothermal system compresses by losing heat to the environment.
The adiabatic process requires two important conditions:
• the system should be isolated from its surroundings; and
• the process must happen swiftly enough to allow for enough time to transfer heat.
In general, the isothermal process can function under two conditions:
•This occurs when the surrounding temperature (T) is less than the temperature of the system (TS), i.e., T < TS, and no thermal equilibrium is maintained.
• This occurs when the external temperature is higher than even the temperatures of the system and thermal equilibrium is not maintained.
Pressure, temperature, and volume are all involved in adiabatic and isothermal processes. They’re all quite clearly drawn with gases as well. In planetary atmospheres, both sorts of processes are crucial.