Final answer:
The statement is false as a positive Gibb's Free Energy indicates a nonspontaneous process, not energy release. A negative Gibb's Free Energy change signifies a spontaneous reaction where energy is released.
Step-by-step explanation:
The statement that Gibb's Free Energy is positive ("+") when energy is released is false. In chemical thermodynamics, Gibb's Free Energy (G) is used to determine the spontaneity of a reaction. The sign of Gibb's Free Energy change (ΔG) indicates whether a reaction is spontaneous or nonspontaneous. Specifically, a negative ΔG indicates a spontaneous process, meaning that it can occur without external energy being added, while a positive ΔG indicates a nonspontaneous process, requiring energy to proceed.
The sign convention is that enthalpy changes (ΔH) are negative if heat is released by the system (exothermic reaction) and positive if heat is absorbed by the system (endothermic reaction). Also, a positive entropy change (ΔS) implies an increase in disorder. When ΔH is negative and ΔS is positive, ΔG will always be negative, indicating a spontaneous reaction at all temperatures. Conversely, when ΔH is positive and ΔS is negative, ΔG will always be positive, and the reaction is never spontaneous.