A reaction has \( \Delta \mathrm{H}=-33 \mathrm{~kJ} \) and \( \Delta \mathrm{S}=-58 \mathrm{~J}...

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A reaction has \( \Delta \mathrm{H}=-33 \mathrm{~kJ} \) and \( \Delta \mathrm{S}=-58 \mathrm{~J} / \mathrm{K} \). This reaction would be:
(a) Spontaneous at all temperatures.
(b) Non-spontaneous at all temperatures.
(c) Spontaneous above a certain temperature.
(d) Spontaneous below a certain temperature.
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