Identifying the Non-State Function Among the Given Options- A Distinguishing Guide
Which of the following is not a state function?
In the field of thermodynamics, understanding the distinction between state functions and path functions is crucial. State functions are properties of a system that depend only on the current state of the system, regardless of how the system arrived at that state. On the other hand, path functions depend on the path taken to reach the state in question. This article aims to identify which of the following options is not a state function.
The first option is the internal energy of a system. Internal energy is a state function because it depends only on the temperature and pressure of the system, not on the process by which it was achieved. Therefore, it is not the correct answer.
The second option is the work done by a system. Work is a path function because it depends on the specific path taken by the system. For instance, the work done by a gas expanding in a cylinder is different if the gas expands slowly compared to if it expands quickly. Hence, this option is a path function and could be the correct answer.
The third option is the heat transferred to a system. Heat transfer is also a path function because it depends on the specific process through which heat is added or removed from the system. The amount of heat transferred can vary depending on the temperature difference between the system and its surroundings. Thus, this option is a path function and could be the correct answer as well.
The fourth option is the change in entropy of a system. Entropy is a state function because it depends only on the current state of the system, not on the path taken to reach that state. Therefore, it is not the correct answer.
In conclusion, the correct answer to the question “Which of the following is not a state function?” is either the second option (work done by a system) or the third option (heat transferred to a system), as both are path functions.