Thermodynamic state functions are path-independent quantities. Explain with an example.

Explanation

A state function is a path-independent quantity. This means that when a system undergoes a process, the change in any state function depends only on the initial and final states of the system, and not on the path of the process. In order to make it clear, let us consider the following process in which 1 mol of an ideal gas undergoes a change in its state: 2 atm, 4L, 273K `to`1 atm, 8L, 273K.
We can make this change by either of the following two proceses. however, in each of these processes, the change in a state function, viz.,P or V is the same.
Process-1: 2 atm, `4L,273Kunderset("expansion")overset("Isothermal")to1` atm, 8L, 273K
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