# Isothermal

Isothermal refers to a process in which a system changes—whether it be the pressure, volume and/or contents—without the temperature changing. From the point of view of the first law of thermodynamics, this means that the internal energy of the system is unchanged, since temperature is a measure of the average kinetic energy of molecules within the system. This then looks like:

and consequently,

where:

• is the change in internal energy
• is heat
• is work

What these equations mean is that the work input to a system must be exactly balanced by a heat output, and vice versa. If an insulated container containing air is compressed (decreasing its volume, positive value), then heat must be removed from the system in accordance (negative value). In contrast, if a container is allowed to expand (negative ), then heat must be added to the system in order to keep the temperature constant. To calculate work, an integration must be done to the formula . This can also be thought of as calculating the area under the curve. However, due to the shape of the curve, it's not as simple of a calculation—in comparison to an isobaric process, for example. The formula below is the integrated equation, and will calculate the work done for any isothermal process:



where:

• is the number of moles
• is the ideal gas constant
• is the initial pressure
• is the final volume

The Carnot efficiency explaining the maximum thermal efficiency of a heat engine is derived by using isothermal processes, in which a thermodynamic cycle is completed with the use of 2 isothermal and 2 adiabatic processes. Phase changes are an example of isothermal processes, since the temperature remains constant until the phase change is complete.

The following video from UC Berkley's chemistry department explains the idea of an isothermal process with visuals.

## Authors and Editors

Kailyn Stenhouse, Jordan Hanania, Bethel Afework, Jason Donev
Last updated: June 25, 2018
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