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State Functions

Posted: Tue Jan 28, 2020 9:38 am
by 605110118
How would you define state functions, and why is enthalpy not considered one?

Re: State Functions

Posted: Tue Jan 28, 2020 10:06 am
by anjali41
A state function is a property of a substance that is independent of how the sample was prepared. According to the textbook definition, it seems that enthalpy is listed as a state function.

Re: State Functions

Posted: Tue Jan 28, 2020 10:12 am
by Jamie Lee 1F
A state function is a property of a system that depends on only the current state, irregardless of what path was taken to get there. Some examples include temperature, pressure, and volume. Enthalpy is considered a state function because it depends on the initial and final states, not the path between.

Re: State Functions

Posted: Wed Jan 29, 2020 8:02 am
by Miriam Villarreal 1J
A state function is a property whose value does not depend on the path taken to reach that specific value. In contrast, functions that depend on the path from two values are call path functions. Both path and state functions are often encountered in thermodynamics.

Re: State Functions

Posted: Wed Jan 29, 2020 8:40 am
by Justin Sarquiz 2F
In addition, enthalpy is a state function because you can add and subtract enthalpy values.

Re: State Functions

Posted: Thu Jan 30, 2020 4:17 pm
by ValerieChavarin 4F
Enthalpy is considered a state function as it is dependent on initial and final states.

Re: State Functions

Posted: Thu Jan 30, 2020 4:48 pm
by Ashley Alvarado 2C
Enthalpy would be considered a state function, meaning it must be able to be added. Change in enthalpy can be added to give the total enthalpy change.

Re: State Functions

Posted: Thu Jan 30, 2020 5:00 pm
by annikaying
A state function is something that is not dependent on how you get to the end result. For enthalpy, it doesn't matter how you get to the value therefore it is a state function. This also implies that state functions are additive.

Re: State Functions

Posted: Thu Jan 30, 2020 7:22 pm
by Uisa_Manumaleuna_3E
My TA explained that when we think of state reactions, it's like asking someone what floor of a building they're on. You say, "What floor are you on?" and the person responds with "first floor" or "second floor" or something like that. In order to know the answer to your question, you don't need to know how long the person was in the elevator or if they stopped to talk to a friend or anything like that.

State functions work just like that. All you want to know is where you started and/or where you ended up. Enthalpy is one of those functions.

Re: State Functions

Posted: Sun Feb 02, 2020 10:38 pm
by kristi le 2F
A state function is a property that depends only on the current state of a system, independent on how the state was prepared. For example, internal energy, pressure, volume, temp, and density are state functions. Work and heat are not.