a)
ΔHo = -58.03 KJ
ΔSo = -176.6 J/K
= -0.1766 KJ/K
T = 298 K
use:
ΔGo = ΔHo - T*ΔSo
ΔGo = -58.03 - 298.0 * -0.1766
ΔGo = -5.4032 KJ
Answer: -5.40 KJ
b)
use:
ΔGo = ΔHo - T*ΔSo
for reaction to be spontaneous, ΔGo should be negative
that is ΔGo<0
since ΔGo = ΔHo - T*ΔSo
so, ΔHo - T*ΔSo < 0
-58.03- T *-0.1766 < 0
T *0.1766 < 58.03
T < 328 K
Answer: Below 328 K
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