- #1
rajakavuru
- 1
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Hello,
If a reaction is spontaneous when calculated using Gibb's Free Energy formula,
Delta G = Delta H - (T*Delta S)
Does it mean the reaction will occur at impossible temperatures even (such as 999999999999999999999999 degrees Kelvin)
for ex:
H2O(g) C(s) --> CO(g)+H2(g)
Delta H = 135.5 kJ
Delta S = .1488 kJ
T = 1173 Kelvin
Delta G = -39 (if delta G is negative, the reaction is spontanious, according to Gibb's Free Energy)
since this reaction is spontanious, will this occur at 99999999999999999 degrees kelvin even? (is this possible?)
If a reaction is spontaneous when calculated using Gibb's Free Energy formula,
Delta G = Delta H - (T*Delta S)
Does it mean the reaction will occur at impossible temperatures even (such as 999999999999999999999999 degrees Kelvin)
for ex:
H2O(g) C(s) --> CO(g)+H2(g)
Delta H = 135.5 kJ
Delta S = .1488 kJ
T = 1173 Kelvin
Delta G = -39 (if delta G is negative, the reaction is spontanious, according to Gibb's Free Energy)
since this reaction is spontanious, will this occur at 99999999999999999 degrees kelvin even? (is this possible?)