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It is not spontaneous.
3600 K
it can never be spontanious
10,267 kJ are needed
-127 KJmol-1
I2(s) --> I2(g); dH=62.4kJ/mol; dS=0.145kJ/mol. The reaction will favor the product at this temperature. Your entropy is positive and your enthalpy is also positive, so this reaction will not be spontaneous at all temperatures. But at room temperature, which is 298K, it will be spontaneous and proceed left to right. (this is the sublimation of iodine)
400 K
It is not spontaneous.
it is never spontaneous
it can never be spontanious
3600 K
G = 0 kJ/mol
It is spontaneous
G= 0 kJ/mol
It can be said to be exothermic since H is negative. Also below a temp of 3708ºC, the reaction will be spontaneous because ∆G will be negative. This is from ∆G = ∆H - T∆S.
it can never be spontanious
H2(g) + S(s) —> H2S + 20.6 kJ