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(B) The spontaneity of a process is determined by the Gibbs free energy equation: $\Delta G = \Delta H - T\Delta S$. For a process to be spontaneous a

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$\Delta H  0$

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(B) The spontaneity of a process is determined by the Gibbs free energy equation: $\Delta G = \Delta H - T\Delta S$. For a process to be spontaneous at all temperatures,$\Delta G$ must be negative $(\Delta G If $\Delta H  0$ (increase in entropy),then $\Delta G = (	ext{negative}) - T(	ext{positive})$. Since $T$ is always positive in Kelvin,$\Delta G$ will always be negative regardless of the temperature $T$.

Which of the following conditions regarding a chemical process ensures its spontaneity at all temperatures?

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