From ΔG = ΔH−TΔS, the 298 K formation entropy is $(416.3-370.7)/298=0.15302$ kJ/(mol K). Under the constant-enthalpy approximation, Gibbs–Helmholtz gives $\Delta G(375)=416.3-375(0.15302)=358.92$ kJ/mol, rounding to 359, A.
More Equilibrium: Laws of thermodynamics. Standard states. Thermochemistry. Thermodynamic functions and their relationships: Gibbs-Helmholtz and Maxwell relations, Gibbs-Duhem equation, Van’t Hoff equation. Criteria of spontaneity and equilibrium. Absolute entropy. Partial molar quantities. Thermodynamics of mixing. Chemical potential. Fugacity, Activity and Activity coefficient. Chemical equilibria. Dependence of equilibrium constant on temperature and pressure. questions
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