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Given: Fe((s))rarrFe^(2+)+2e^(-), E^(@)=...

Given: `Fe_((s))rarrFe^(2+)+2e^(-), E^(@)=+0.44V`
`Pb_((s))rarrPb^(2+)+2e^(-),E^(@)=+0.13V`
`Ag^(+)+e^(-)rarrAg,E^(@)=+0.8V`
`Cu^(2+)+2e^(-)rarrCu,E^(@)=+0.34V`
Which of the following metal ion will oxidise iron?

A

`Ag^(+)` only

B

`Cu^(2+)` only

C

`Pb^(+2)` only

D

All

Text Solution

Verified by Experts

The correct Answer is:
C
`Fe^(2+) + 2e^(-) to Fe, E^(@) =-0.44 V`
`Pb^(2+) + 2e^(-) to pb, E^(@) = -0.13 V`
`Ag^(+) + e^(-) to Ag, E^(@) = +0.8 V`
`Cu^(2+) + 2e^(-) to Cu, E^(@) = +0.34 V`
SRP values of pb, Ag, Cu are higher than Fe, So, pb, Ag, Cu oxidises Fe
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