Question

What is the standard potential of the cell \(\text{Ni} \, | \, \text{Ni}^{2+}(1\,\text{M}) \, || \, \text{Cu^{2+}(1\,\text{M}) \, | \, \text{Cu}\) if \(E^\circ_{\text{Cu}^{2+}/\text{Cu}} = 0.337\ \text{V}\) and \(E^\circ_{\text{Ni}^{2+}/\text{Ni}} = -0.236\ \text{V}\)?}

• A. 0.101 V
• B. –0.136 V
• C. 0.573 V
• D. –0.753 V

Hint:

Always subtract anode potential from cathode potential to find cell emf.

Answer 1

The Correct Option is C

Step 1: Identify cathode and anode.
Copper has a higher standard reduction potential, so it acts as the cathode.
Nickel acts as the anode.

Step 2: Use cell potential formula.
\[ E^\circ_{\text{cell}} = E^\circ_{\text{cathode}} - E^\circ_{\text{anode}} \]

Step 3: Substitute the given values.
\[ E^\circ_{\text{cell}} = 0.337 - (-0.236) \]
\[ E^\circ_{\text{cell}} = 0.573\ \text{V} \]

Step 4: Conclusion.
The standard potential of the cell is \(0.573\ \text{V}\).