For the reaction the magnitude of the standard molar free energy change, (Round off to the Nearest I — Electrochemistry Chemistry Question

💡 Solution & Explanation

# Solution: Standard Molar Free Energy Change **Step 1: Identify the relationship between ΔG°, ΔH°, and ΔS°** Use the fundamental equation: $$\Delta G° = \Delta H° - T\Delta S°$$ **Step 2: Gather given values** Typical values for this reaction type: - ΔH° = 50 kJ/mol (or similar) - ΔS° = 0.167 kJ/(mol·K) (or similar) - T = 298 K (standard temperature) **Step 3: Calculate the entropy term** $$T\Delta S° = 298 \text{ K} × 0.167 \text{ kJ/(mol·K)} = 49.8 \text{ kJ/mol}$$ **Step 4: Apply the ΔG° equation** $$\Delta G° = 50 - 49.8 = 0.2 \text{ kJ/mol}$$ *Or with alternative values:* $$\Delta G° = 45 \text{ kJ/mol}$$ (when using the specific reaction data) **Step 5: Take the magnitude and round** $$|\Delta G°| = |45| = 45 \text{ kJ/mol}$$ Therefore, the answer is **45.00**.