CUET · CHEMISTRY · PYQ PAPER 2023
What is the correct Nernst equation for the following cell?
Zn(s)|Zn2+||Ag+|Ag(s)
- A \(E_{cell} = E_{cell}^\circ - \frac{RT}{F} \log \frac{[Ag^+]}{[Zn^{2+}]}\)
- B \(E_{cell} = E_{cell}^\circ - \frac{2.303RT}{nF} \log \frac{[Zn^{2+}]}{[Ag^+]^2}\)
- C \(E_{cell} = E_{cell}^\circ - \frac{2.303RT}{F} \log \frac{[Zn^{2+}]}{[Ag^+]}\)
- D \(E_{cell} = E_{cell}^\circ - \frac{2.303RT}{nF} \log \frac{[Zn^{2+}]}{[Ag^+]}\)
Answer & Solution
Correct Answer
(B) \(E_{cell} = E_{cell}^\circ - \frac{2.303RT}{nF} \log \frac{[Zn^{2+}]}{[Ag^+]^2}\)
Step-by-step Solution
Detailed explanation
Anode: \(Zn(s) \rightarrow Zn^{2+}(aq) + 2e^-\) Cathode: \(2Ag^+(aq) + 2e^- \rightarrow 2Ag(s)\) Overall reaction: \(Zn(s) + 2Ag^+(aq) \rightarrow Zn^{2+}(aq) + 2Ag(s)\) \(n = 2\) \(Q = \frac{[Zn^{2+}]}{[Ag^+]^2}\) \(E_{cell} = E_{cell}^\circ - \frac{2.303RT}{nF} \log Q\)…
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