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The standard electrode potential for the...

The standard electrode potential for the half cell reactions are
`Zn^(2+)+2e^(-)rarrZn ,E^(@)=-0.76V`
`Fe^(2+)+2e^(-)rarrFe,E^(@)=-0.44V`
The EMF of the cell reaction
`Fe^(2+)+ZnrarrZn^(++)+Fe` is

A

`-0.32V`

B

`-1.20V`

C

`+1.20V`

D

`+0.32V`

Text Solution

Verified by Experts

The correct Answer is:
D
`Fe^(2+)+ZnrarrZn^(2+)+Fe`
`ZnrarrZn^(2+)+2e^(-)`
`ZnrarrZn^(2+)+2e^(-)`
`Fe^(2+)+2e^(-)rarrFe`
`Zn|Zn^(2+)||Fe^(2+)|Fe`
`EMF^(@)=E_(Fe^(2+)//Fe)^(@)-E_(Zn^(2+)//Zn)^(@)`
`=-0.44-(-0.76)`
`=0.76-0.44=+0.32V`
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Electrode potential for the following half-cell reactions are Zn rarr Zn^(2+)+2e^(-), E^(@)=+0.76V, Fe rarr Fe^(2+)+2e^(-), E^(@)=+0.44V The EMF for the cell reaction Fe^(2+)+Zn rarr Zn^(2+)+Fe will be

The standard oxidation potential E^(@) for the half cell reactions are Zn rarrZn^(2+)+2e^(-):E^(@)=+0.76V FerarrFe^(2+)+2e^(-)"E^(@)=+0.41V EMF of the cell reaction Fe^(2+)+ZnrarrZn^(2+)+Fe will be

The standard electrode potential of the half cells are given below. ZnrarrZn^(2+)+2e^(-):E^(@)=0.76V FerarrFe^(2+)+2e^(-):E^(@)=0.44V The emf of the cell Fe^(2+)+ZnrarrZn^(2+)+Fe is

The standard oxidation potential E^@ for the half cell reaction are Zn rarr Zn^2+2e^- E^@=+ 0.76 V Fe rarr Fe^2+ + 2e^- E^@=+ 0.41 V EMF of the cell rection is Zn+Fe^(2+) rarr Zn^(2+)+Fe

The standard reductino potentials E^(c-) for the half reactinos are as follows : ZnrarrZn^(2+)+2e^(-)" "E^(c-)=+0.76V FerarrFe^(2+)+2e^(-) " "E^(c-)=0.41V The EMF for the cell reaction Fe^(2+)+Znrarr Zn^(2+)+Fe is

The standared reduction potntial E^o for the half-reactions are as. Zn=Zn^(2+) + 2 e^- , E^o = + 76 V Fe = Fe^(2+) + 2e^- , E^o = + 0.41 V . The EMF for cell recaction Fe^(2+) = Zn rarr Zn^(2+) + Fe is.

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