A state function is a function whose value depends only on the state of the system, not on how the system arrived at that state.
The correct answer and explanation is:
The correct answer is: True.
A state function is indeed a property of a system that is determined only by its current state and is independent of the path taken to reach that state. The value of a state function depends solely on the current conditions of the system, such as pressure, temperature, and volume, rather than on how those conditions were achieved.
State functions are crucial in thermodynamics because they allow the prediction of a system’s behavior without needing to consider the detailed process that led to its present state. Examples of state functions include internal energy (U), enthalpy (H), entropy (S), and Gibbs free energy (G). These quantities are independent of the path taken from one state to another and only depend on the initial and final states.
For instance, consider the internal energy of a gas. If a gas undergoes a process where it expands from one state to another, the change in its internal energy depends only on the initial and final states, such as its temperature and pressure. Whether the gas undergoes a slow compression or a rapid expansion, the change in internal energy remains the same. This is a defining feature of state functions.
In contrast, path-dependent functions like work (W) and heat (Q) do depend on the specific way the system undergoes a process. Work, for example, will vary depending on how a system is compressed or expanded, while heat depends on the specifics of heat transfer during a process.
The distinction between state functions and path-dependent functions is fundamental in thermodynamics, as it allows scientists and engineers to focus on system properties at any given moment without needing to track every detail of its history.