Distinguish between isothermal and adiabatic process?

Question: Distinguish between isothermal and adiabatic process?

An isothermal process and an adiabatic process are two different types of thermodynamic processes that describe how a system changes its state. Here's how they can be distinguished:

Isothermal Process:

- In an isothermal process, the temperature of the system remains constant throughout the entire process.

- The system is in thermal equilibrium with its surroundings, meaning there is a continuous heat exchange to maintain the temperature.

- During an isothermal process, the system absorbs heat from the surroundings when work is done on it, and it releases heat to the surroundings when work is done by it.

- The change in internal energy of the system is zero, as the temperature remains constant.

- On a pressure-volume (P-V) diagram, an isothermal process is represented by a hyperbolic curve.

Adiabatic Process:

- In an adiabatic process, there is no heat exchange between the system and its surroundings.

- The system is thermally isolated, meaning there is no transfer of heat during the process.

- As a result, the temperature of the system can change during an adiabatic process.

- An adiabatic process can occur when the system is well-insulated or when the process happens rapidly, allowing no time for heat exchange.

- The change in internal energy of the system is determined by the work done on or by the system.

- On a P-V diagram, an adiabatic process is represented by a steeper curve compared to an isothermal process.

In summary, an isothermal process maintains a constant temperature by exchanging heat with the surroundings, while an adiabatic process does not exchange heat and allows for changes in temperature.

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