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yarga [219]
3 years ago
12

For a reaction to be nonspontaneous under standard conditions at all temperatures, the signs of δh∘ and δs∘ must be ________ and

________, respectively.
Chemistry
1 answer:
8090 [49]3 years ago
6 0
For a reaction to be nonspontaneous under standard conditions at all temperatures, the signs of ΔH and ΔS must be positive and negative, respectively.
<span>Gibbs free energy (G) determines if reaction will proceed spontaneously.
</span><span>ΔG = ΔH - T·ΔS.</span>
ΔG - changes in Gibbs free energy.<span>
ΔH - changes in enthalpy.
ΔS - changes in entropy.
T is temperature in Kelvins.
When ΔS < 0 (negative entropy change) and ΔH > 0 (endothermic reaction), the process is never spontaneous (<span>ΔG> 0).
</span></span>
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