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 . These two couples in their standard state are connected to make a cell. The cell potential will be
  1. $+0.89 \mathrm{~V}$
  2. $+0.18 \mathrm{~V}$
  3. $+1.83 \mathrm{~V}$
  4. $+1.199 \mathrm{~V}$

Solution

$\begin{aligned} & E_{\mathrm{Sn}^{4+} / \mathrm{Sn}^{2+}}^{\circ} \mathrm{V} \\ & E_{\mathrm{CI}^{3+} / \mathrm{Cr}}^{\circ}=-0.74 \mathrm{~V} \\ & E_{\text {cell }}^{\circ}=E_{\text {cathode }}^{\circ}(R P)-E_{\text {anode }(\mathrm{RP})}^{\circ} \\ &=0.15-(-0.74) \\ &=+0.89 \mathrm{~V} . \end{aligned}$

Asked in: NEET 2011 (Screening)

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