Why do you define Enthalpy as a state function?

Question

Well, in my chemistry note says that a state function is described by means of macroscopic properties and the enthalpy change is a state function. But for example in ionization, you get gaseous atoms first which are then converted to gaseous ions but you can't observe a macroscopic change (electron clouds!?!).

But by referring Hess's law I can see that the enthalpy change is a state function in energetic aspect.

Please describe briefly.

Answer 1

A state function is one in which the only things that is important are the initial and final conditions. In other words, the path taken to reach the final state from the initial state is irrelevant.



It is known that work is not a state function. That is, the amount of work done to accomplish a task will depend upon the path taken to do the work.



In the link below there is a figure that shows different pathways taken to react Na and Cl to produce NaCl. In this case the enthalpy of the reaction is dependent on only the initial and final states of the reactants and products.



Hope this is helpful to you.

Answer 2

warmth is a path functionality because of the fact it relies upon on the strain for the period of heating/cooling and not in user-friendly terms the preliminary and extremely final temperatures and pressures. Enthalpy is a state functionality because of the fact it relies upon in user-friendly terms on the preliminary and extremely final states of the equipment. it rather is autonomous of tension because of the fact ?H is often measured at consistent tension (if it have been measured at changing tension, we'd call it q, no longer ?H). power is a state functionality because of the fact it relies upon in user-friendly terms on the preliminary and extremely final states of the equipment.

Answer 3

See link. It might give you some insight.

http://www.google.com/search?q=define:enthalpy&nomo=1