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KonstantinChe [14]
3 years ago
7

For a reaction to be spontaneous under standard conditions at all temperatures, the signs of δh° and δs° must be __________ and

__________, respectively.
Chemistry
1 answer:
Shalnov [3]3 years ago
8 0
For a reaction to be spontaneous under standard conditions at all temperatures, the signs of ΔH° and ΔS° must be negative and positive, respectively.
<span>Gibbs free energy (G) determines if reaction will proceed spontaneously, if </span>ΔG is negative, reaction is spontaneous.<span>
ΔG = ΔH - T·ΔS.
ΔG - changes in Gibbs free energy.
ΔH - changes in enthalpy.
ΔS - changes in entropy.
T is temperature in Kelvins.</span>

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<h2>1.54 mL</h2>

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3 0
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*
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