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CUET · CHEMISTRY · PYQ PAPER 2025

The standard Gibbs energy of the following reaction is \(-610 kJ mol ^{-1}\)
\(Mg(s)+2 Ag^{+}(aq) \rightarrow Mg^{2+}(aq)+2 Ag(s)\)
What is the standard EMF for the cell correspondng to the above reaction?
Given: Faraday's constant \(=96500 C mol ^{-1}\)

  1. A -6.32 V
  2. B +6.32 V
  3. C +3.16 V
  4. D -3.16 V
Verified Solution

Answer & Solution

Correct Answer

(C) +3.16 V

Step-by-step Solution

Detailed explanation

\(E^\circ = -\frac{\Delta G^\circ}{nF}\) \(E^\circ = -\frac{-610 \times 10^3 \text{ J mol}^{-1}}{2 \times 96500 \text{ C mol}^{-1}}\) \(E^\circ = +3.16 \text{ V}\)
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