CUET · CHEMISTRY · PYQ PAPER 2023
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 \(=96500 C mol ^{-1}\)
- A -6.32 V
- B +6.32 V
- C +3.16 V
- D -3.16 V
Answer & Solution
Correct Answer
(C) +3.16 V
Step-by-step Solution
Detailed explanation
\(E^\circ_{cell} = \frac{-\Delta G^\circ}{nF}\) \(E^\circ_{cell} = \frac{-(-610 \times 10^3 \text{ J mol}^{-1})}{2 \times 96500 \text{ C mol}^{-1}}\) \(E^\circ_{cell} = +3.16 \text{ V}\)
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