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MHT CET · Chemistry · Electrochemistry

What is value of \(E_{\text {cell }}\) at 298 K for the reaction, \(\mathrm{Zn}_{(\mathrm{s})}+\mathrm{Cu}^{+2}(0 \cdot 1 \mathrm{M}) \rightarrow \mathrm{Zn}^{+2}(0 \cdot 1 \mathrm{M})+\mathrm{Cu}_{(\mathrm{s})}\) if \(\mathrm{E}_{\text {cell }}^{\circ}=1 \cdot 1 \mathrm{~V}\) ?

  1. A 1.1 V
  2. B 0.11 V
  3. C 1.0408 V
  4. D 0.0296 V
Verified Solution

Answer & Solution

Correct Answer

(A) 1.1 V

Step-by-step Solution

Detailed explanation

\(E_{\text{cell}} = E_{\text{cell}}^{\circ} - \frac{0.0592}{n} \log Q\) \(Q = \frac{[\mathrm{Zn}^{+2}]}{[\mathrm{Cu}^{+2}]} = \frac{0 \cdot 1}{0 \cdot 1} = 1\)
From MHT CET
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