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Calculate E(cell)^(@) for the following ...

Calculate `E_(cell)^(@)` for the following reaction at 298 K:
`2AI(s) + 3Cu^(2+)(0.01M) to 2A1^(3+)(0.01M) + 3Cu(s)`
`"Given" : E_(cell) = 1.98V`
(b) Using the `E^(@)` values A and B, predict which is better for coating the surface of iron
`[E^(@)(Fe^(2+)//Fe) = -0.44V]` to prevent corrosion and why?
`"Given" : E^(@)(A^(2+)//A) = 2.37V : E^(@)(B^(2+) //B) = 0.14V`

Text Solution

Verified by Experts

Metals of lower electrode potential value when connected with iron protect it form oxidation and prevent corrosion. Hence, coating of metal A having lower electrode potential will be better than B which has higher `E_((b^(2+//B))^(@) =-0.14V`.
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Knowledge Check

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