1)
ΔH = -683 KJ
ΔS = -366 J/K
= -0.366 KJ/K
use:
ΔG = ΔH - T*ΔS
For K to be greater than 1, reaction should be spontaneous.
for reaction to be spontaneous, ΔG should be negative
that is ΔG<0
since ΔG = ΔH - T*ΔS
so, ΔH - T*ΔS < 0
-683.0- T *-0.366 < 0
T *0.366 < 683.0
T < 1866 K
Answer: Below 1866 K
2)
ΔH = 181 KJ
ΔS = 24.9 J/K
= 0.0249 KJ/K
use:
ΔG = ΔH - T*ΔS
For K to be greater than 1, reaction should be spontaneous.
for reaction to be spontaneous, ΔG should be negative
that is ΔG<0
since ΔG = ΔH - T*ΔS
so, ΔH - T*ΔS < 0
181.0- T *0.0249 < 0
T *0.0249 > 181.0
T > 7269 K
Answer: Above 7269 K
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