Problem: 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/molB  ΔG°f = +529.5 kJ/molC ΔG°f = +402.0 kJ/molPart 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 leftb) entropy-driven to the leftc) entropy-driven to the rightd) enthalpy-driven to the right

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Problem Details

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°= +387.7 kJ/mol

B  ΔG°= +529.5 kJ/mol

C ΔG°= +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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