It is not spontaneous.
it can never be spontanious
-127 KJmol-1
3600 K
10,267 kJ are needed
I think you should try and use q = mcT where q = heat change m = mass of substance c = specific heat capacity of the substance ( Water is 4.187 kJmol-1) T = change in temperature (oC) so for your question, q = mcT q = 12 x 4.187 x (93-15.4) q = 3898.9344 kJmol-1 Hope this helps!!
G = 0 kJ/mol
G= 0 kJ/mol
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)
it can never be spontanious
400 K
it is never spontaneous
H2(g) + S(s) —> H2S + 20.6 kJ
It is spontaneous
it can never be spontanious
just add them together and you get 147kj
group 1
-127 KJmol-1