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MHT CET · Chemistry · Electrochemistry

\(\text {Calculate } \mathrm{E}_{\text {cell }}^{\circ} \text { for } \mathrm{Cd}_{(\mathrm{s})}\left|\mathrm{Cd}_{(\mathrm{IM})}^{++}\right|\left|\mathrm{Ag}_{(\mathrm{MM})}^{+}\right| \mathrm{Ag}_{(\mathrm{s})}.\) \(\ {\left[\mathrm{E}_{\mathrm{Cd}}^{\circ}=-0.403 \mathrm{~V} ; \mathrm{E}_{\mathrm{Ag}}^{\circ}=0.799 \mathrm{~V}\right]}\)

  1. A \(1.202 V\)
  2. B \(-1.202 V\)
  3. C \(0.396 V\)
  4. D \(-0.396 V\)
Verified Solution

Answer & Solution

Correct Answer

(A) \(1.202 V\)

Step-by-step Solution

Detailed explanation

For the given cell, anode is \(\mathrm{Cd}\) and cathode is Ag.
\(\begin{aligned}
\mathrm{E}_{\text {cell }}^{\circ} & =\mathrm{E}_{\text {cathode }}^{\circ}-\mathrm{E}_{\text {anode }}^{\circ} \\
& =0.799-(-0.403) \\
& =1.202 \mathrm{~V}
\end{aligned}\)