Standard electrode potential for $\mathrm{Sn}^{4+} / \mathrm{Sn}^{2+}$ couple is $+0.15 \mathrm{~V}$ and…

Standard electrode potential for $\mathrm{Sn}^{4+} / \mathrm{Sn}^{2+}$ couple is $+0.15 \mathrm{~V}$ and that for the $\mathrm{Cr}^{3+} / \mathrm{Cr}$ couple is $-0.74 \mathrm{~V}$. These two couples in their standard state are connected to make a cell. The cell potential will be:
  1. $+1.19 \mathrm{~V}$
  2. $+0.89 \mathrm{~V}$
  3. $+0.18 \mathrm{~V}$
  4. $+1.83 \mathrm{~V}$

Solution

Given $\mathrm{E}_{\mathrm{Sn}^{4+} / \mathrm{Sn}^{2+}}=+0.15 \mathrm{~V}$
$\mathrm{E}_{\mathrm{Cr}^{3+}} / \mathrm{Cr}=-0.74 \mathrm{~V}$
$E_{\text {cell }}^{\mathrm{o}}=\mathrm{E}_{\text {cathode }}^{\mathrm{o}}-\mathrm{E}_{\text {anode }}^{\mathrm{o}}$
$=0.15-(-0.74)=+0.89 \mathrm{~V}$ .

Asked in: JEE-TOPICTESTS-CHEMISTRY

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