Which of the following best describes what happens to the standard entropy change, ΔS∘, of an elementary reaction when the reaction is written in the reverse direction?
a) ΔS∘ is multiplied by −T, where T is the absolute temperature.
b) ΔS∘ is unchanged because entropy is a state function.
c) ΔS∘ keeps the same magnitude but its sign is reversed.
d) ΔS∘ is divided by Avogadro’s number to account for reversed stoichiometry.