Consider an electrochemical cell with a zinc electrode immersed in 1.0 M Zn²⁺ and a nickel electrode immersed in 0.10 M Ni²⁺.
Zn²⁺ + 2e- $\to$ Zn
$\varepsilon$ ° = -0.76 V
Ni²⁺ + 2e- $\to$ Ni
$\varepsilon$ ° = -0.23 V
-Calculate the concentration of Ni²⁺ if the cell is allowed to run to equilibrium at 25°C.

Question

Consider an electrochemical cell with a zinc electrode immersed in 1.0 M Zn²⁺ and a nickel electrode immersed in 0.10 M Ni²⁺.
Zn²⁺ + 2e-

\to

Zn

\varepsilon

° = -0.76 V
Ni²⁺ + 2e-

\to

Ni

\varepsilon

° = -0.23 V
-Calculate the concentration of Ni²⁺ if the cell is allowed to run to equilibrium at 25°C.

Quizplus · Accepted Answer

The question involves a calculation that cannot be completed as provided due to the presence of placeholder symbols (like ²⁺, F1F1F1S1, etc.) instead of chemical formulas and numbers. These placeholders prevent the application of the Nernst equation or any other relevant electrochemical calculations to determine the concentration of Ni²⁺ at equilibrium.

Consider an Electrochemical Cell with a Zinc Electrode Immersed in 1.0