Chemistry

Chemistry

Problem

Consider the following standard free-energy changes: Reaction I: X →\rightarrow Y ΔG∘=+15.0 kJ mol−1\Delta G^{\circ}=+15.0\,\text{kJ}\,\text{mol}^{-1} Reaction II: Y →\rightarrow Z ΔG∘=−32.0 kJ mol−1\Delta G^{\circ}=-32.0\,\text{kJ}\,\text{mol}^{-1} What is ΔG∘\Delta G^{\circ} for the overall conversion X →\rightarrow Z? a) +17.0 kJ mol−1+17.0\,\text{kJ}\,\text{mol}^{-1} b) −17.0 kJ mol−1-17.0\,\text{kJ}\,\text{mol}^{-1} c) −47.0 kJ mol−1-47.0\,\text{kJ}\,\text{mol}^{-1} d) −32.0 kJ mol−1-32.0\,\text{kJ}\,\text{mol}^{-1}

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