Final answer:
The reaction of converting copper(II) sulfide to copper(II) sulfate is spontaneous under standard conditions as indicated by a negative Gibbs free energy change of -608.316 kJ.
Step-by-step explanation:
To determine if the conversion of copper(II) sulfide (CuS) to copper(II) sulfate (CuSO₄) is spontaneous under standard conditions, we can use the values of enthalpy change (ΔH°rxn) and entropy change (ΔS°rxn) provided to calculate the Gibbs free energy change (ΔG°rxn) using the Gibbs free energy equation:
ΔG°rxn = ΔH°rxn - TΔS°rxn
Given that ΔH°rxn = -718.3 kJ and ΔS°rxn = -368 J/K for the reaction:
CuS(s) + 2O₂(g) → CuSO₄(s)
We will have the calculate ΔG°rxn at room temperature (25°C or 298K).
ΔG°rxn = -718.3 kJ - (298 K)(-368 J/K × 1 kJ/1000 J)
ΔG°rxn = -718.3 kJ + 109.984 kJ = -608.316 kJ
The negative value of ΔG°rxn indicates that the reaction is spontaneous under standard conditions.