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Chemistry
Corrosion of iron is essentially an electro chemical phenomenon where the cell reactions are:
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Q. Corrosion of iron is essentially an electro chemical phenomenon where the cell reactions are:
KCET
KCET 2022
A
$Fe$ is oxidized to $Fe ^{3+} \& H_2 O$ is reduced to $O ^{22-}$
B
$Fe$ is oxidized to $Fe^{ 2+}\& H_2 O$ is reduced to $O _{2}-$
C
$Fe$ is oxidized to $Fe ^{2+}\& H_2 O$ is reduced to $OH$ - ions
D
$Fe$ is oxidized to $Fe^{3+}\& H_2 O$ is reduced to $O_2$
Solution:
Explanation: The rusting of iron is $Fe \rightleftarrows Fe ^{2+}+2 e ^{-}$(oxidation)
$H _{2} O +1 / 2 O _{2}+2 e ^{-} \rightleftarrows 2 OH ^{-} \text {(reduction) }$