Part A: Use the data given here to calculate the values of ΔG°rxn (kJ/mol) at 25 °C for the reaction described by the equation:
A + B ⇌ C
A ΔG°f = +387.7 kJ/mol
B ΔG°f = +529.5 kJ/mol
C ΔG°f = +402.0 kJ/mol
Part B: If ΔH°rxn and ΔS°rxn are both positive values, what drives the spontaneous reaction and in what direction at standard conditions?
a) enthalpy-driven to the left
b) entropy-driven to the left
c) entropy-driven to the right
d) enthalpy-driven to the right
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