Question

For the cell reaction \( 2\text{Cu}^{2+} + \text{Co} \rightarrow 2\text{Co}^{2+} + \text{Cu} \), \( E^\circ_{\text{cell}} \) is 1.89V. If \( E^\circ_{\text{Co}^{2+}/\text{Co}} \) is -0.28V, what is the value of \( E^\circ_{\text{Cu}^{2+}/\text{Cu}} \)?

• A. 0.28V
• B. 1.61V
• C. 2.17V
• D. 1.0V

Hint:

The standard electrode potentials can be used to calculate the cell potential by using the formula \( E^\circ_{\text{cell}} = E^\circ_{\text{cathode}} - E^\circ_{\text{anode}} \).

Answer 1

The Correct Option is B

Step 1: Using the Nernst equation.
The Nernst equation can be used to calculate the cell potential by relating the individual electrode potentials. We can find the value of \( E^\circ_{\text{Cu}^{2+}/\text{Cu}} \) using the given values.

Step 2: Conclusion.
The value of \( E^\circ_{\text{Cu}^{2+}/\text{Cu}} \) is 1.61V, corresponding to option (2).