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For the given reactions
Sn2+ + 2e−-− →\to→ Sn
Sn4+ + 4e−-− →\to→ Sn
the electrode potentials are ; ESn2+/Sno=−0.140E_{S{n^{2 + }}/Sn}^o = - 0.140ESn2+/Sno=−0.140 V and ESn4+/Sno=+0.010E_{S{n^{4 + }}/Sn}^o = + 0.010ESn4+/Sno=+0.010 V. The magnitude of standard electrode potential for Sn4+/Sn2+S{n^{4 + }}/S{n^{2 + }}Sn4+/Sn2+ i.e. ESn4+/Sn2+oE_{S{n^{4 + }}/S{n^{2 + }}}^oESn4+/Sn2+o is _____________ ×\times× 10−-−2 V. (Nearest integer)
Sn ⟶ Sn2++2 e− E10=0.140 V\mathrm{Sn} \longrightarrow \mathrm{Sn}^{2+}+2 \mathrm{e}^{-} \quad \mathrm{E}_{1}^{0}=0.140 \mathrm{~V}Sn ⟶ Sn2++2 e− E10=0.140 V
Sn4++4 e− ⟶ Sn E20=0.010 V \mathrm{Sn}^{4+}+4 \mathrm{e}^{-} \longrightarrow \mathrm{Sn} \quad \mathrm{E}_{2}^{0}=0.010 \mathrm{~V} Sn4++4 e− ⟶ Sn E20=0.010 V
Sn4++2 e− ⟶ Sn2+ E cell 0 EcellO=n2 E2o+n1 E10n=4(0.010)+2(0.140)2 E cell 0=0.16 V=16 × 10−2 V \begin{aligned} & \mathrm{Sn}^{4+}+2 \mathrm{e}^{-} \longrightarrow \mathrm{Sn}^{2+} \quad \mathrm{E}_{\text {cell }}^{0} \\ & \mathrm{E}_{\mathrm{cell}}^{\mathrm{O}}=\frac{\mathrm{n}_{2} \mathrm{E}_{2}^{\mathrm{o}}+\mathrm{n}_{1} \mathrm{E}_{1}^{0}}{\mathrm{n}}=\frac{4(0.010)+2(0.140)}{2} \\ & \mathrm{E}_{\text {cell }}^{0}=0.16 \mathrm{~V}=16 \times 10^{-2} \mathrm{~V} \end{aligned} Sn4++2 e− ⟶ Sn2+ E cell 0 EcellO=nn2 E2o+n1 E10=24(0.010)+2(0.140) E cell 0=0.16 V=16 × 10−2 V
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