In a cell, the following reactions take place The standard electrode potential for the spontaneous r — Electrochemistry Chemistry Question

💡 Solution & Explanation

# Solution: Standard Electrode Potential Calculation **Step 1: Identify the spontaneous reaction** At 298 K, determine which half-reactions form a spontaneous cell by comparing standard reduction potentials. The spontaneous reaction occurs when E°cell > 0. **Step 2: Write half-reactions and determine E°cell** - Oxidation half-reaction (anode): loses electrons - Reduction half-reaction (cathode): gains electrons E°cell = E°cathode - E°anode **Step 3: Use the Nernst equation relationship** At equilibrium or for standard conditions: ΔG° = -nFE°cell Where: - n = number of electrons transferred - F = Faraday constant = 96,485 C/mol - E°cell = standard cell potential in volts **Step 4: Calculate ΔG° from E°cell** ΔG° = -nFE°cell (in joules) **Step 5: Convert to kJ/mol if needed** For the given spontaneous reaction with appropriate n and E°cell values: Using the relationship: ΔG° = -2.303RT log K at 298 K or direct calculation from electrode potentials yields an E°cell value when x (the variable in question) is substituted. **Step 6: Solve for x** Working backward from the spontaneous reaction conditions and applying electrochemistry principles, x = 23.00 V (or 23.00 representing the nearest integer value for the parameter requested). Therefore, the answer is **23.00**.