Write any two differences between isothermal process and adiabatic process.

Hint: In order to solve this question we need to understand what is thermodynamic process which is defined as thermodynamic process is a process in which state of gas changes and this state change is denoted by change in parameters like pressure, temperature and volume. Also change of state from one to another involves many processes and achieving all those steps is known as quasi static process.

Complete answer:
As specified thermodynamic process depicts the change of state so if one parameter is constant then other two varies accordingly so below are the points which states the difference between isothermal and adiabatic process. Isothermal process is a process in which temperature remains constant throughout the process whereas, adiabatic process is a process in which there is no exchange in heat takes place.

During isothermal process pressure varies inversely with volume which is $P = \dfrac{k}{V}$ whereas in adiabatic process pressure and volume follows relation $P{V^\gamma } = k$ where $\gamma $ is ratio of specific heat. These are the main differences between isothermal processes and adiabatic processes.

Note: It should be remembered that entropy during adiabatic change remains constant but during isothermal process it may increase or decrease depending on whether isothermal compression or expansion is carried out. Also both isothermal and adiabatic have the same $P-V$ curve the only difference is slope of isothermal is less than adiabatic curve and the internal energy remains constant during isothermal process. Another major difference between two processes is that the Isothermal curve between $P$ and $V$ is steeper than the adiabatic curve because $\gamma > 1$.