Free energy, G=- TS, is a state funtion that indicates whether a reaction is spontaneous or non-spontaneous if you think of TS as the part of the system's energy that is discordered already, then (H-TS) is the part of system's energy that is still orderd and therefore free to cause spontaneous change by becoming disorder Also, `Delta G = Delta H - T Delta S`
Form the second law of thermodyamics, a reaction is spontaneous if `Delta _("total") S ` is + ve, nonspontaneous if `Delta _("total")S` is negative and at equilibrium if `Delta_(lot)S` is zero. Since, `- T Delta S= Delta C` and since `Delta G and Delta S` have oposite single we can restate the themodynmaic creation for the spontaneity of a reaction oout at constant temperature and pressure.
If `Delta G lt 0,` the reaction is spontaneous. `If Delta G gt 0,` the reaction is non-spontaneous.
If `Delta G =0,` the reaction is at equilibrium.
A particular reaction has a negative value for the free enregy charge. Then at ordinary temmperature

Options

A. It has a large `(-ve)` value for the entropy change
B. It has a large (+ve) value for enthalpy change
C. It has a small (+ve) value for enthalpy change
D. It has a (+ve) value for the entropy change and a (-ve) value for enthalpy change

Explanation

`Delta G= Delta H - T DeltaS` can be negative at ordinary temperature T if `Delta H` is - ve and `Delta S` is + ve.