Corrosion of iron is essentially an electrochemical phenomenon where the cell reactions are

Question

Corrosion of iron is essentially an electrochemical phenomenon where the cell reactions are (A) Fe is oxidised to Fe 2+ and dissolved oxygen in water is reduced to H 2 O (B) Fe is oxidised to Fe 3+ and O 2 is reduced to O 2 2- (C) Fe is oxidised to Fe 2+ and O 2 is reduced to O 2- (D) Fe is oxidised to Fe 2+ and O 2-is reduced to O 2-2

Tardigrade Admin · Accepted Answer

Correct answer is (a) Fe is oxidised to Fe 2+ and dissolved oxygen in water is reduced to H 2 O

Q. Corrosion of iron is essentially an electrochemical phenomenon where the cell reactions are

$F e$ is oxidised to $F e^{2 +}$ and dissolved oxygen in water is reduced to $H_{2} O$

$F e$ is oxidised to $F e^{3 +}$ and $O_{2}$ is reduced to $O_{2}^{2 -}$

$F e$ is oxidised to $F e^{2 +}$ and $O_{2}$ is reduced to $O_{2}^{-}$

$F e$ is oxidised to $F e^{2 +}$ and $O_{2}^{-}$ is reduced to $O_{2}^{- 2}$

Correct answer is (a) $F e$ is oxidised to $F e^{2 +}$ and dissolved oxygen in water is reduced to $H_{2} O$

Q. Corrosion of iron is essentially an electrochemical phenomenon where the cell reactions are

Fe is oxidised to Fe2+ and dissolved oxygen in water is reduced to H2​O

Fe is oxidised to Fe3+ and O2​ is reduced to O2​2−

Fe is oxidised to Fe2+ and O2​ is reduced to O2−​

Fe is oxidised to Fe2+ and O2−​is reduced to O2−2​

Correct answer is (a) Fe is oxidised to Fe2+ and dissolved oxygen in water is reduced to H2​O

$F e$ is oxidised to $F e^{2 +}$ and dissolved oxygen in water is reduced to $H_{2} O$

$F e$ is oxidised to $F e^{3 +}$ and $O_{2}$ is reduced to $O_{2}^{2 -}$

$F e$ is oxidised to $F e^{2 +}$ and $O_{2}$ is reduced to $O_{2}^{-}$

$F e$ is oxidised to $F e^{2 +}$ and $O_{2}^{-}$ is reduced to $O_{2}^{- 2}$

Correct answer is (a) $F e$ is oxidised to $F e^{2 +}$ and dissolved oxygen in water is reduced to $H_{2} O$