Given that :

$E_{A g^{+} / A g}^{0} = + 0.80 V E_{C o^{2 +} / C o}^{0} = - 0.28 V E_{C u^{2 +} / C u}^{0} = + 0.34 V E_{Z n^{2 +} / Z n}^{0} = - 0.76 V$

Which of the following metal has the highest rate of corrosion ?

A g

No worries! We‘ve got your back. Try BYJU‘S free classes today!

C u

No worries! We‘ve got your back. Try BYJU‘S free classes today!

C o

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Z n

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

Open in App

Solution

The correct option is D $Z n$
Metals on corrosion form oxide layer on the surface i.e. gets oxidised.

$A g$ oxidises to $A g_{2} O$ .Here oxidation state changes from 0 to +1
$C o$ oxidises to $C o O$ . Here oxidation state changes from 0 to +2
$C u$ oxidises to $C u O$ . Here oxidation state changes from 0 to +2
$Z n$ oxidises to $Z n O$ . Here oxidation state changes from 0 to +2

The metal which has the highest oxidation potential will form the oxide much faster and thus get corroded most easily.
Since,
$E_{Z n / Z n^{2 +}}^{0}$ is the highest. So, corrosion of $Z n$ is the fastest

Suggest Corrections

Similar questions

E_{A g^{+} / A g}^{0}

E_{C u^{2 +} / C u}^{0}

E_{F e {3 +}^{+} / F e 2 +}^{0}

E_{C e {4 +}^{+} / C e 3 +}^{0}

Given: $E_{A g^{\oplus} | A g}^{⊖} = + 0.80 V; E_{C o^{2 +} | C o}^{⊖} = - 0.28 V,$

$E_{C u^{2 +} | C u}^{⊖} = + 0.34 V, E_{Z n^{2 +} | Z n}^{⊖} = - 0.76 V$

Which metal will corrode fastest?

{C u}_{(s)} + {2 A g}_{(a q)}^{+} ⟶ {C u}_{(a q)}^{2 +} + {2 A g}_{(s)}

E_{A g^{+} / A g}^{0} = 0.80 V, E_{C u^{2 +} / C u}^{0} = 0.34 V .

Δ G

Z n_{(s)} + A g_{2} O_{(s)} + H_{2} O_{(l)} \to Z n_{(a q)}^{2 +} + 2 A g_{(s)} + 2 O H^{-}_{(a q)}

E_{{A g}^{+} / A g}^{0} = + 0.80 V

E_{{Z n}^{+ 2} / Z n}^{0} = - 0.76 V

Join BYJU'S Learning Program