Derivation of Enthalpy
Derivation of Enthalpy
(OP)
Having difficulty deriving the following
(d(G/T))/(d(1/T) is apparently equal to H? ( G, Gibbs Free Energy, T, Temperature , H, Enthalpy - referring to partial differential keeping V constant)
How is this so? Any help would be helpful!!
(d(G/T))/(d(1/T) is apparently equal to H? ( G, Gibbs Free Energy, T, Temperature , H, Enthalpy - referring to partial differential keeping V constant)
How is this so? Any help would be helpful!!





RE: Derivation of Enthalpy
Since [∂(G/T)/∂T]p = - H/T2, it follows that
[∂(G/T)/∂(1/T)]p = H
RE: Derivation of Enthalpy
In a similar manner with the Helmholtz free energy A
Since [∂(A/T)/∂T]v = - U/T2, it follows that
[∂(A/T)/∂(1/T)]v = U
where U is the internal energy, v is volume, and p is pressure (previous posting).
RE: Derivation of Enthalpy
RE: Derivation of Enthalpy
With Hemlholz function
a=u-Ts>a/T=u/T-s>d(a/T)=d(u/T)-ds
(skipped a few steps) d(a/T) =du/T-udT/T^2-ds
since ds=du/T+Pdv/T
d(a/T)= -udT/T^2-Pdv/T
let v=constant
d(a/T)=-udT/T^2
since d(1/T)=-dT/T^2
d(a/t)/d(1/T)=u
RE: Derivation of Enthalpy
To jrv24, this is conventional information appearing in books on thermodynamics. You may see from the above messages that the definition you are seeking is not true.
To chicopee, use the Process TGML Step 2 option when writing a message.