Given the standard reduction potentials for the following half-cells: Co²⁺(aq) + 2e⁻ Co(s) E^ = -0.28 V Au³⁺(aq) + 3e⁻ Au(s) E^ = +1.40 V Which of the following correctly represents the IUPAC notation for the spontaneous electrochemical cell formed by these half-cells and its standard cell potential?

Step-by-step solution

For a spontaneous electrochemical cell, the standard cell potential E^ _ cell must be positive. The half-cell with the higher standard reduction potential acts as the cathode (reduction), and the one with the lower standard reduction potential acts as the anode (oxidation). Given: E^ _ Au³⁺/Au = +1.40 V E^ _ Co²⁺/Co = -0.28 V Since +1.40 V > -0.28 V, the Au³⁺/Au half-cell undergoes reduction at the cathode, and the Co²⁺/Co half-cell undergoes oxidation at the anode. According to IUPAC convention, the cell is repres