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According to the 2nd law of thermodynamics, a spontaneous process will occur (or rather: is very likely to occur) if [tex] \Delta S > 0[/tex].
A chemical process occurs if [tex] \Delta G < 0[/tex], where [tex] G = H - TS[/tex].
Example:
H = -100 kJ
T = 1 K
S = -10 kJ/K
so [tex] \Delta G = - 190 kJ[/tex]. In this example, [tex] \Delta G < 0[/tex] but [tex] \Delta S < 0[/tex].
Doesn't this contradict the 2nd law?
A chemical process occurs if [tex] \Delta G < 0[/tex], where [tex] G = H - TS[/tex].
Example:
H = -100 kJ
T = 1 K
S = -10 kJ/K
so [tex] \Delta G = - 190 kJ[/tex]. In this example, [tex] \Delta G < 0[/tex] but [tex] \Delta S < 0[/tex].
Doesn't this contradict the 2nd law?