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

Question

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] · Answer 1 · 2022-02-10T19:58:54+03:00

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>