Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C.(The equation is balanced.) 2 K(s) + I₂(s) → 2 K⁺(aq) + 2 I⁻(aq)
K⁺(aq) + e⁻ → K(s) E° = -2.93 V
I₂(s) + 2 e⁻ → 2 I⁻(aq) E° = +0.54 V

Question

Quizplus · Accepted Answer

The cell potential can be calculated using the formula: E°cell = E°reduction of Cathode - E°reduction of Anode where cathode is where reduction occurs and anode is where oxidation occurs. In this case, reduction occurs at the cathode where I₂(s) is reduced to I⁻, and oxidation occurs at the anode where K(s) is oxidized to K⁺. Therefore, E°cell = (+0.54 V) - (-2.93 V) E°cell = +3.47 V Note that the sign of each half-cell potential must be considered in the calculation to obtain the correct sign of the cell potential.

Use the Standard Half-Cell Potentials Listed Below to Calculate the Standard