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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

  • Calculate the reduction potential for the following half cell reaction at 298 K. Ag^(+)(aq)+e^(-)toAg(s) "Given that" [Ag^(+)]=0.1 M and E^(@)=+0.80 V

    A
    0.741 V
    B
    0.80 V
    C
    `-0.80`V
    D
    `-0.741`V

  • Calculate DeltaG^(@) for the reaction : Cu^(2+)(aq) +Fe(s) hArr Fe^(2+)(aq) +Cu(s) . Given that E^(@)Cu^(2+)//Cu = 0.34 V , E_(Fe^(+2)//Fe)^(@) =- 0.44 V

    A
    11.44 kJ
    B
    180.8 kJ
    C
    150.5 kJ
    D
    28.5 kJ
    • VMC MODULES ENGLISH-ELECTROCHEMISTRY-Level-0 (Very short Answer Type )(1Marks)
    1. Calculate E(cell)^(@) for the following reaction at 298 K: 2AI(s) +...

      Text Solution

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