$$\ce{XY2 -> X + Y2} \hskip{2em} \Delta H^\circ = \pu{50 kJ/mol_{rxn}}$$

The equation above represents the decomposition of a compound $\ce{XY2}$. The reaction is thermodynamically favorable under standard conditions at 298 K. Therefore, the value of $\Delta S^\circ$ for the reaction must be

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$$\Delta G^\circ = \Delta H^\circ - T \Delta S^\circ$$

For a reaction to be thermodynamically favorable, $\Delta G^\circ \lt 0$.

$$\Delta H^\circ - T \Delta S^\circ \lt 0$$ $$\Delta H^\circ \lt T \Delta S^\circ$$ $$\frac{\Delta H^\circ}{T} \lt \Delta S^\circ$$