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Complete amateur here. When looking at one form of the equation deriving the change in Gibbs free energy for a given chemical reaction, the terms change in enthalpy, and the negative product of temperature (in kelvin) and change in entropy:
$$\Delta G = \Delta H - T\,\Delta S$$
This seems to double count how temperature will influence the spontaneity of the reaction if temperature is already considered when deriving entropy, $S$.
Any guidance would be appreciated.
One reason we write equations this way is because all of the parameters on the right-hand-side can be measured or computed independently.
Consider an analogous (but more intuitive) equation, the Stokes-Einstein relation for the diffusion coefficient $D$ of a particle in a liquid:
$$D = \frac{k_\mathrm{B} T}{6\pi\eta r}$$
where $\eta$ is the dynamic viscosity, $r$ is the radius of the particle, and $k_\mathrm{B}$ is Botzmann's constant. Here we see an explicit dependence of $D$ on $T$, but there is also an implicit dependence on $T$ through $\eta$ and possibly also $r$. Is this a problem? No, assuming the equation holds and we can determine the parameters accurately at each $T$ of interest. Whether that is a simple thing is another question.
Also, it is fair to wonder to what extent the parameters are fundamentally independent, or, whether by digging into the gory details of atomic structure of matter, we might not find $r$ and $\eta$ to be connected in some other way. But that is another question.
Even if the final temperature of the products is the same as the initial temperature of the reactants, you can still have a change in entropy, enthalpy, and Gibbs free energy of products relative to the reactants. This is the result of making and breaking chemical bonds and not the result of a temperature change. Entropy and enthalpy are not just functions of temperature (and pressure), but also chemical makeup. In such a well-defined case, there would certainly not be any double counting of the temperature.
