Question

For an exothermic process which is spontaneous:

• A. $\Delta G$ may be positive
• B. $\Delta G$ must be positive
• C. $\Delta G$ must be zero
• D. temperature must be over $500K$
• E. $\Delta G$ must be negative

Answer 1

The correct option is E $\Delta G$ must be negative

For an exothermic process which is spontaneous, $\Delta G$ must be negative.
Low enthalpy and high entropy are driving spontaneous reactions, these leads to negative value of gibbs free energy change.
$\Delta G=\Delta H-T\Delta S$