Question

If the emf of cell, \(\text{Cu}_{(s)}|\text{Cu}_{(1M)}^{2+}|\text{Ag}_{(1M)}^+|\text{Ag}\) is 0.463 V at \(25 ^{\circ}\text{C}\) and standard potential of Cu electrode is 0.337 V. Find the standard potential of Ag electrode

• A. \(0.128 \text{V}\)
• B. \(-0.128 \text{V}\)
• C. \(0.8 \text{V}\)
• D. \(-0.8 \text{V}\)

Hint:

At 1 M both ions, \(E_{cell} = E^{\circ}_{cathode} - E^{\circ}_{anode}\).

Answer 1

The Correct Option is C

Step 1: Write the half reactions
Anode: Cu $\to$ Cu$^{2+}$ + 2e$^-$. Cathode: Ag$^+$ + e$^-$ $\to$ Ag.

Step 2: Add potentials
$E_{cell} = E_{\text{red (cathode)}} + E_{\text{oxid (anode)}} = E^{\circ}_{Ag} - 0.337 = 0.463$, so $E^{\circ}_{Ag} = 0.8$ V, option (C).

Final Answer:
The standard electrode potential of Ag is 0.8 V, option (C). \[ \boxed{0.8\ \text{V}} \]