Thermochemistry ( enthalpy and heat )
Can anyone explain why is it that heat which is generally a path function, becomes a state function when constant pressure condition is present (enthalpy)
I@Dexter
INote for OP
+solved @user1 @user2... to close the thread when your doubt is solved. Mention the users who helped you solve the doubt. This will be added to their stats.
Ilemme give you another example. work is a path func but reversible work is a state function 
Iheat is a path fn
Iheat at const v is also a state fn - energy
Iit is what it is is all i am saying, we acknowledge is and use it to manipulate energy
DSo does that mean, that if we specify some conditions, we observe that the value of heat becomes associated with just the ideas of initial and final states and consequently we acknowledged the fact and said enthalpy that is heat at constant pressure is state function because we observe it to be so,there is no how it’s just what it is in nature, did I get it right or I missed something
DOk got it sir @iTeachChem, I was just wondering that maybe constant pressure had some implications at a higher level concept or something, I think my doubt has been clarified, thank you
Citeachchem
Transcription requested by DarkWhite
and see Delta E which is a state function is a summation of Q plus W both of it apart functions. There's another one.
D+solved @iTeachChem
IPost locked and archived successfully!
Archived by
@1205127026940452884 (1205127026940452884)
Time
June 5, 2024
Solved by
@1035556259417571408 (1035556259417571408)
