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at 298 K For the reaction: 2NO2 (g)N2s (e) The value of AHo and Aso are-58.03 kJ and -176.6 J/K, respectively (a) What is the

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Answer #1

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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