Rachit Garg said:internal energy is path function so work done in an adiabiatic process should also be path function
Rachit Garg said:why work done in adibiatic reversible and irreversible different?
Rachit Garg said:By mistake i have wriitten that i want to say In an adiabiatic process q=0 so change in internal energy become equal to work. Since internal energy is state function so work done in an adiabiatic process should also be state function then why work done in adibiatic reversible and irreversible different?
An adiabatic process is a thermodynamic process in which there is no heat transfer between the system and its surroundings. This means that the change in internal energy of the system is equal to the work done on it.
The equation q=0 means that there is no heat transferred during the process. This is a defining characteristic of an adiabatic process and is what sets it apart from other thermodynamic processes.
Work done is considered a path function in an adiabatic process because its value depends on the path taken to reach a certain state, rather than just the initial and final states of the system. This is because the amount of work done on a system is affected by external factors such as pressure and volume, which can vary along different paths.
The first law of thermodynamics states that the change in internal energy of a system is equal to the heat added to the system minus the work done by the system. In an adiabatic process, q=0, so the equation simplifies to ΔU = -W. This means that the change in internal energy is solely dependent on the work done on the system.
Some common examples of adiabatic processes include the expansion or compression of gases in a piston, the flow of air over an airplane wing, and the compression of air in a bicycle pump. These processes occur without any heat transfer, making them adiabatic.