We have the Gibbs Helmholtz equation:
ΔG = ΔH - TΔS
(279.62 kJ) = ΔH - (156.7+273) x (253.74 x 10-3 kJ/K)
ΔH = (279.62 kJ) + (109.0 kJ)
ΔH = 388.65 kJ
Apply the same equation at T = 3.7oC
ΔG = ΔH - TΔS
ΔG = (388.65 kJ)- (3.7+273) x (253.74 x 10-3 kJ/K)
ΔG = (388.65 kJ) - (70.21 kJ)
ΔG = 318.44 kJ ------------------ (ANSWER)
For a particular reaction at 156.7 °C, AG = 279.62 kJ, and AS = 253.74 J/K....
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