3)
A)
ΔHrxn = 150.0 KJ
ΔSrxn = 100 J/K
= 0.1 KJ/K
use:
ΔGrxn = ΔHrxn - T*ΔSrxn
for reaction to be spontaneous, ΔGrxn should be negative
that is ΔGrxn<0
since ΔGrxn = ΔHrxn - T*ΔSrxn
so, ΔHrxn - T*ΔSrxn < 0
150.0- T *0.1 < 0
T *0.1 > 150.0
T > 1500 K
Answer: high temperatures
B)
ΔHrxn = 200.0 KJ
ΔSrxn = -100 JK
= -0.1 KJ/K
use:
ΔGrxn = ΔHrxn - T*ΔSrxn
for reaction to be spontaneous, ΔGrxn should be negative
that is ΔGrxn<0
since ΔGrxn = ΔHrxn - T*ΔSrxn
so, ΔHrxn - T*ΔSrxn < 0
200.0- T *-0.1 < 0
T *0.1 < -200.0
T < -2000 K
Since kelvin temperature can't be negative
The reaction will never be spontaneous
Answer: NO TEMPERATURES
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