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On the basis of the following E^(@) val...

On the basis of the following `E^(@)` values, the strongest oxidizing agent is :
`[Fe(CN)_(6)]^(4-) to [Fe(CH)_(6)j]^(3)+ +e ^(-),E^(@)=-0.35 V`
`Fe ^(32+)+e ^(-)," "E ^(@)=-0.77V`

A

`,Fe(CN)_(6)]^(4)`

B

`Fe ^(2+)`

C

`Fe ^(3+)`

D

`[Fc(CN)_(6)]^(3+)`

Text Solution

Verified by Experts

The correct Answer is:
C
From the given data we find `Fe ^(3+)` is strongest oxidising agent. More the positive value of `E ^(@).` more is the tendency to get oxidized. Thus correct option is (c).
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On the basis of the following E^(@) values, the stongest oxidizing agent is [Fe(CN)_(6)]^(4-) rarr [Fe(CN)_(6)]^(3-)+e^(-), E^(@) = -0.35 V Fe^(2+) rarr Fe^(3+)+e^(-), E^(@) = -0.77 V

On the basis of the folwing E^@ values, the strongest oxidizing agent is [Fe(CN)_6 ]_4^(-) rarr [Fe(CN)_5]^(3-) +3^- , E^@ =- 0.35 V Fe^(2+) rarr Fe^(3+) + e^(- : E^@ =- 0. 77 V .

On the basis of the standard electrode potential velues, state whether Ti^(4+) species can be used to oxidise Fe(II) to Fe(III). Ti^(4+)+e^(-) to Ti^(3+)," "E^(@)=+0.1 V Fe^(3+)+e^(-) to Fe^(2+)," "E^(@)=+0.77 V

(i) On the basis of the standard electrode potential values stated for acid solutions, predict whether Ti^(4+) species may be used to oxidise Fe(II) to Fe(III) {:(Ti^(4+) + e^(-) to Ti^(3+), E^(@) = +0.01V), (Fe^(3+) + e^(-) to Fe^(2+), E^(@)= +0.77V):} (ii) Based on the data arrange Fe^(3+), Mn^(2+) " and " Cr^(2+) in the increasing order of stability of +2 oxidation state. (Give a brief reason) E_(Cr^(3+)//Cr^(2+))^(@) = -0.4V E_(Mn^(3+)//Mn^(2+))^(@) = +1.5V E_(Fe^(3+)//Fe^(2+))^(@) = +0.8V

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