Zinc is used to protect iron from corrosion because:

E_{r e d}

Z n < E_{r e d}

of iron

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E_{o x i d a t i o n}

Z n < E_{o x i d a t i o n}

of iron

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E_{o x i d a t i o n}

Z n = E_{o x i d a t i o n}

of iron

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zinc is cheaper than iron

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Solution

The correct option is A $E_{r e d}$ of $Z n < E_{r e d}$ of iron
Zinc is used to protect iron from corrosion because it is more active metal than iron and it has more tendency to lose electrons with respect to iron. In other words, zinc has a negative reduction potential higher than that of iron.

$E_{z n^{2 +} | Z n}^{o} = - 0.76 V$

$E_{F e^{2 +} | F e}^{o} = - 0.44 V$

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Similar questions

2 A g^{+} + C_{6} H_{12} O_{6} + H_{2} O \to 2 A g (s) + C_{6} H_{12} O_{7} + 2 H^{+}

A g^{+} + e^{-} \to A g; E_{r e d}^{o} = 0.8 V C_{6} H_{12} O_{6} + H_{2} O \to C_{6} H_{12} O_{7} + 2 H^{+} + 2 e^{-}; E_{r e d}^{o} = - 0.05 V A g (N H_{3})_{2}^{+} + e^{-} \to A g (s) + N H_{3}; E_{r e d}^{o} = 0.337 V

Z n

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