The standard electrode potential of the half cells are given below - Zn2-2e- Zn- E1 - -7-62 V Fe2-2e- Fe- E2 - -7-81 VThe emf of the cell- Fe2-Zn- Zn2-Fe is-

The correct option is A 0.19 V Zn^2++2e^ → n; E_1 = 7.62 V #160; #160; #160; #160; #160; #160; —— E_1 Fe^2++2e^ → Fe; E_ ...

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EMF

The standard ...

Question

The standard electrode potential of the half cells are given below -

$Z n^{2 +} + 2 e^{-} \to Z n; E_{1} = - 7.62 V$

$F e^{2 +} + 2 e^{-} \to F e; E_{2} = - 7.81 V$

The emf of the cell, $F e^{2 +} + Z n \to Z n^{2 +} + F e$ is:

1.52 V

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- 1.54 V

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- 0.19 V

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0.19 V

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Similar questions

Z n^{2 +} + 2 e^{-} \to Z n; E = - 0.76 V

F e^{2 +} + 2 e^{-} \to F e; E = - 0.44 V

F e^{2 +} = Z n^{-} \to Z n^{2 +} + F e

E^{o}

Z n \to Z n^{2 +} + 2 e^{-}; E^{o} = - 0.76 V

F e^{2 +} + 2 e^{-} \to F e; E^{o} = + 0.41 V

F e^{2 +} + Z n \to Z n^{2 +} + F e

E^{o}

Z n ⟶ {Z n}^{2 +} + 2 e^{-}

E^{o} = + 0.76 V

F e ⟶ {F e}^{2 +} + 2 e^{-}

E^{o} = + 0.41 V

{F e}^{2 +} + Z n ⟶ {Z n}^{2 +} + F e

Z n \to Z n^{2 +} + 2 e^{-} (E_{(Z n^{2 +} / Z n)}^{0} = - 0.76 V)

F e \to F e^{2 +} + 2 e^{-} E^{0} = 0.41 V

F e^{2 +} + Z n \to Z n^{2 +} + F e

E^{\circ}

Z n \to Z n^{2 +} + 2 e^{-}; E^{\circ} = + 0.76 v o l t

F e \to F e^{2 +} + 2 e^{-}; E^{\circ} = + 0.41 v o l t

F e^{2 +} + Z n \to Z n^{2 +} + F e

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