Question

how can a reaction with a negative value of $delta g^{0}$ be described?
a. as spontaneous
b. as endothermic
c. as exothermic
d. as nonspontaneous

Explanation:

The Gibbs - free energy change ($\Delta G^0$) determines the spontaneity of a reaction. A negative $\Delta G^0$ indicates that the reaction will proceed spontaneously under standard conditions. Endothermic and exothermic refer to heat - absorption and heat - release respectively, which are related to $\Delta H$. Non - spontaneous reactions have positive $\Delta G^0$ values.

Answer:

A. As spontaneous