Hess's Law

[Diana Chavez-Carrillo 2L]

Since Hess's Law can be used for both enthalpy and entropy since they are both state functions and extensive properties, why is there no delta on the S for entropy as shown by its equation: ∆S°rxn = ∑ S° products - ∑ S° reactants but there is one for enthalpy: ∆H°rxn = ∑ ∆H° f products - ∑ ∆H° f reactants?

[Adam Kramer 1A]

I believe that it has the same relationship as Hess's law because they are both state functions (entropy and enthalpy), but they are not exactly the same because Hess's law only applies to enthalpy. There is a very similar relationship, but they are different because we cannot track H alone. It is usually written as delta H because it is a relative measurement from the previous state to the next, unlike entropy, which we can track in its current state.

[Diana Chavez-Carrillo 2L]

I believe that it has the same relationship as Hess's law because they are both state functions (entropy and enthalpy), but they are not exactly the same because Hess's law only applies to enthalpy. There is a very similar relationship, but they are different because we cannot track H alone. It is usually written as delta H because it is a relative measurement from the previous state to the next, unlike entropy, which we can track in its current state.

Oh, I see! Wow, that makes more sense thank you so much for clarifying that!