Given E deg(Ni^2+/Ni) = -0.25 V and E deg(Sn^2+/Sn) = -0.14 V. For the cell Ni | Ni^2+ (1 M) || Sn^2+ (1 M) | Sn, the standard EMF and the anode are

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Given $E^{\circ} (Ni X^{2 +} / Ni) = - 0.25 V$ and $E^{\circ} (Sn X^{2 +} / Sn) = - 0.14 V$ . For the cell $Ni ∣ Ni X^{2 +} (1 M) ∣∣ Sn X^{2 +} (1 M) ∣ Sn$ , the standard EMF and the anode are

E_{cell}^{\circ} = E_{cathode}^{\circ} - E_{anode}^{\circ}

. The electrode with lower (more negative)

E^{\circ}

is the anode, so Ni is oxidised.

E_{cell}^{\circ} = - 0.14 - (- 0.25) = 0.11 V

, positive, so the cell works as written. Adding the two values (

0.39 V

) is the common error.