Zinc can be coated on iron to produce galvanized iron but the reverse is not possible. It is because

Question

Zinc can be coated on iron to produce galvanized iron but the reverse is not possible. It is because (A) zinc is lighter than iron (B) zinc has lower melting point than iron (C) zinc has lower negative electrode potential than iron (D) zinc has higher negative electrode potential than iron

Tardigrade Admin · Accepted Answer

E0Zn+2/Zn = - 0.76 V E0Fe+2 /Fe = - 0.76 V Zn has higher negative SRP (Standard reduction potential) so it works as anode and protect iron to make iron as cathode.

Q. Zinc can be coated on iron to produce galvanized iron but the reverse is not possible. It is because

zinc is lighter than iron

zinc has lower melting point than iron

zinc has lower negative electrode potential than iron

zinc has higher negative electrode potential than iron

$E_{Z n^{+ 2} / Z n}^{0} = - 0.76 V$
$E_{F e^{+ 2} / F e}^{0} = - 0.76 V$
Zn has higher negative SRP (Standard reduction potential) so it works as anode and protect iron to make iron as cathode.

Q. Zinc can be coated on iron to produce galvanized iron but the reverse is not possible. It is because

zinc is lighter than iron

zinc has lower melting point than iron

zinc has lower negative electrode potential than iron

zinc has higher negative electrode potential than iron

EZn+2/Zn0​=−0.76V EFe+2/Fe0​=−0.76V Zn has higher negative SRP (Standard reduction potential) so it works as anode and protect iron to make iron as cathode.

$E_{Z n^{+ 2} / Z n}^{0} = - 0.76 V$
$E_{F e^{+ 2} / F e}^{0} = - 0.76 V$
Zn has higher negative SRP (Standard reduction potential) so it works as anode and protect iron to make iron as cathode.