Final answer:
The standard cell potential (E°cell) for the electrochemical cell is calculated to be 1.537 V by subtracting the standard anode potential from the standard cathode potential. To obtain the nonstandard cell potential, adjustments for reactant and product concentrations would typically be made using the Nernst equation, but the necessary details for this calculation were not provided.
Step-by-step explanation:
To determine the nonstandard cell potential for an electrochemical cell, we first need to write down the given half-reactions and their standard electrode potentials (E°). The reactions given are:
- Ni2+(aq, 2.0 M) + 2 e− → Ni(s), with E° = −0.26 V (anode)
- ClO2(aq, 0.010 M) + H+(aq, 1.0 M) + e− → HClO2(aq, 2.0 M) + H2O(l), with E° = 1.277 V (cathode)
To find the overall standard cell potential (E°cell), use the formula:
E°cell = E°cathode - E°anode
In this case, E°cell = 1.277 V - (-0.26 V) = 1.537 V.
Since we are not operating under standard conditions, we would need to account for the concentrations of the reactants and products using the Nernst equation to calculate the actual cell potential. However, as no specific details or instruction to use the Nernst equation were provided in this question, the determination of the nonstandard cell potential cannot be completed.