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Zinc is used ...

Question

Zinc is used to protect iron from rusting. This is because:

E_{r e d .}^{\circ}

of zinc is greater than that of

F e

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E_{o x .}^{\circ}

Z n

is greater than that of

F e

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E_{r e d .}^{\circ}

Z n

is nearly equal to that of

F e

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Z n

is cheap

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Solution

The correct option is C $E_{o x .}^{\circ}$ of $Z n$ is greater than that of $F e$
$\to$ The rusting of iron can be prevented by coating the metal surface with another metal such as Zinc, that is oxidized in preference to iron.
$\to Z n$ is stronger reducing agent than $F e$ and thus can be oxidized easily than $F e$ .
$F e_{(a q)}^{2 +} + 2 e^{-} \to F e_{(s)} E^{\circ} = - 0.44 V$
$Z n_{(a q)}^{2 +} + 2 e^{-} \to Z n_{(s)} E^{\circ} = - 0.763 V$

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Similar questions

E_{c e l l}^{0}

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

E_{Z n / Z n^{+ 2}}^{0} = 0.76 V, E_{F e / F e^{+ 2}}^{0} = + 0.41 V

E^{o}

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

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

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

E_{O_{Z n}}^{0} < E_{O_{F e}}^{0}

E_{O_{S n}}^{0} > E_{O_{F e}}^{0}

E^{o}

Z n \to Z n^{2 +} + 2 e^{-}, E^{\circ} = + 0.76 V F e \to F e^{2 +} + 2 e^{-}, E^{\circ} = + 0.41 V

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

Standard reduction potential values for the electrodes are given below.

$M g^{2 +} + 2 e^{-} \to M g;$ $E_{r e d}^{o} =$ $- 2.37$ V

$Z n^{2 +} + 2 e^{-} \to Z n;$ $E_{r e d}^{o} =$ $- 0.76$ V

$F e^{2 +} + 2 e^{-} \to F e;$ $E_{r e d}^{o} =$ $- 0.44$ V

Which of the following statement is correct ?

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