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The standard oxidation potentials, , fo...

The standard oxidation potentials, , for the half reactions are as follows :
`Zn rightarrow Zn^(2+) + 2e^(-)` ,` E^(@) = +0.76V`
`Fe rightarrow Fe^(2+)+ 2e^(-), E^(@) = + 0.41 V`
The EMF for the cell reaction,
`Fe^(2+) + Zn rightarrow Zn^(2+) + Fe`

A

`-0.35 V`

B

`+0.35 V `

C

`+1.17 V`

D

`-1.17 V`

Text Solution

Verified by Experts

The correct Answer is:
B
`E^(@) = E_("red")^(@) ("cathode") - E_("red")^(@) ("anode")`
`= E_(Fe^(2+) //Fe)^(@) - E_(Zn^(2+)// Zn)^(@)`
`= -0.41 - (-0.76) = 0.35 V `
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The standard oxidation potential, E^(@) , for the reactions are given as: Zn rightarrow Zn^(2+) + 2e^(-) , E^(@) = +0.76V Fe rightarrow Fe^(2+) + 2e^(-) , E^(@) = +0.41V The emf for the cell : Fe^(2+) + Zn rightarrow Zn^(2+) + Fe

The standard reduction potential E^(@) for the half reactions are as : E^(@) Znrightarrow Zn^2+),E^(@) = +0.76V Fe rightarrow Fe^(2+)+ 2e^(-), E^(@) = 0.41V , The emf for the cell reaction, Fe^(2+)+ZnrightarrowZn^(2+) + Fe is ,

The standard oxidation potentials, E^(@) , for the half reactions are as, Zn rarr Zn^(2+) + 2e^(-), " " E^(@) = + 0.76 volt Fe rarr Fe^(2+) + 2e^(-), " " E^(@) = +0.41 volt The emf of the cell, Fe^(2+) + Zn rarr Zn^(2+) + Fe is:

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The standard reduction potential E^(@) , for the half reaction are : {:(Zn rarr Zn^(2+) + 2e^(-),,,E^(@) = 0.76 V),(Cu rarr Cu^(2+) + 2e^(-),,,E^(@) = 0.34 V):} The emf for the cell reaction, Zn(s)+Cu^(2+) rarr Zn^(2+) + Cu(s) is :

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