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Given E(Cr^(3+)//Cr)^(@)=-0.72V, and E...

Given `E_(Cr^(3+)//Cr)^(@)=-0.72V`, and
`E_(Fe^(2+)//Fe)^(@)=-0.42V`
The potential for the cell.
`Cr|Cr^(3+)(0.1M)||Fe^(2+)( 0. 01M)Fe` is

A

0.339V

B

`0.339V`

C

`-0.26V`

D

0.26V

Text Solution

Verified by Experts

The correct Answer is:
D
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Given E_(Cr^(3+)//Cr)^(@)= 0.72V , E_(Fe^(2+)//Fe)^(@)=-0.42V . The potential for the cell Cr|Cr^(3+)(0.1M)||Fe^(2+) (0.01M) | Fe is :

Given : E_(Fe^(3+)//Fe)^(@) = -0.036V, E_(FE^(2+)//Fe)^(@)= -0.439V . The value of electrode potential for the change, Fe_(aq)^(3+) + e^(-)rightarrow Fe^(2+) (aq) will be :

Knowledge Check

  • Given E_(Cr^(3+)//Cr)^(@)=-0.72V. E_(Fe^(2+)//Fe)^(@)=-0.42V The potential for the cell, Cr|Cr^(3+) (0.1M)||Fe^(2+) (0.01M)|Fe is

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    B
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    C
    0.339V
    D
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  • Given E_(Cr^(3+)//Cr)^(@)=-0.72 V, E_(Fe ^(2+)//Fe)^(@)=-0.42V. The potential for the cell Cr|Cr^(3l) (0.1M)||Fr ^(2l)(0.01M)|Fe is

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    B
    `0.336V`
    C
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    D
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  • Given E_(Cr^(3+)//Cr)^(o)=-0.72V,E_(Fe^(2+)//Fe)^(o)=-0.42V . The potential for the cell Cr|Cr^(3+)(0.1M)||Fe^(3+)(0.01M)|Fe is

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    B
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    C
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    D
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    Calculate the e.m.f. of the cell, Cr//Cr^(3+)(0.1 M) || Fe^(2+)(0.01 M)//Fe "Given" : E_(Cr^(3+)//Cr)^(@)=-0.75" V ", E_(Fe^(2+)//Fe)^(@)=-0.45" V " "Cell reaction" : 2Cr(s)+3Fe^(2+)(aq) to 2Cr^(3+)(aq)+3Fe(s) {"Hint". E_(cell)=E_(cell)^(@)-(0.0591V)/(6)"log"([Cr^(3+)]^(2))/([Fe^(2+)]^(3)}

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