paragchitnis said:The terms internal energy, enthalpy, entropy are state functions. Are change in internal energy([itex]\Delta[/itex]U or [itex]\Delta[/itex]E),change in enthalpy([itex]\Delta[/itex]H) and change in entropy([itex]\Delta[/itex]S) state functions?
State functions in thermodynamics are physical properties that depend only on the current state of a system, and not on how the system reached that state. They include variables such as temperature, pressure, and volume.
Unlike state functions, path functions depend on the path taken to reach a particular state of a system. Examples of path functions include work and heat, which are affected by the specific process used to change the state of a system.
State functions are important because they allow us to describe and analyze thermodynamic systems in a simplified manner. By focusing on state functions, we can make predictions and calculations without needing to know the details of the processes involved.
No, state functions do not change as long as the system remains in the same state. This means that the value of a state function will remain constant even if the system undergoes a change in other variables.
The first and second laws of thermodynamics apply to state functions. For example, the first law 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, and this is true for any process that keeps the system in the same state.