Home
Class 12
CHEMISTRY
Given electrode potentials are , Fe^(3+)...

Given electrode potentials are , `Fe^(3+) + e to Fe^(2+), E^@ = 0.771V " " I_2 + 2e to 2I^(-), E^@ = 0.536 V`,
`E^@` cell for the cell reaction, `2Fe^(3+) + 2I^(-) to 2Fe^(2+) + I_2` is

A

`(2xx0.771-0.536)=1.006V`

B

`(0.771-0.5xx0.536)=0.503V`

C

`(0.771-0.536)=0.235V`

D

`(0.536-0.771)=0.236V`

Text Solution

Verified by Experts

The correct Answer is:
c
`E^(c-)._(cell)=E^(c-)._(o x i d)+E^(c-)._(red)=-0.536+0.771=0.236V`
Promotional Banner

Similar Questions

Explore conceptually related problems

The standard electrode potentials E^(@) for the half cell reactions are as : ZntoZn^(2+)+2e^(-),E^(@)=0.76V FetoFe^(2+)+2e^(-),E^(@)=041V The EMF of the cell reaction Fe^(2+)+ZntoZn^(2+)+Fe is :

E^(@) for a cell having, Fe to Fe^(2+) + 2e, E^(@) = 0.40 V Zn to Zn^(2+) +2e, E^(@) = 0.76 V

Standard electrode potentials are : Fe^(2+) "|" Fe (E^(@) = - 0.44 V), Fe^(3+) "|" Fe^(2+) (E^(@) = 0.77 V) Fe^(2+), Fe^(3+) and Fe blocks are kept together, then

Standard electrode potentials are : Fe^(2+) "|" Fe (E^(@) = - 0.44 V), Fe^(3+) "|" Fe^(2+) (E^(@) = 0.77 V) Fe^(2+), Fe^(3+) and Fe blocks are kept together, then

If E ^(@) (Fe ^(2+)|Fe)=-0.441 V and E ^(@) (Fe ^(3+) |Fe ^(2+))=0.77 1V, the standard E.M.F. of the reaction : Fe + 2F e ^(3+) to 2F e ^(2+) will be

In a simple electrochemical cell, the half cell reduction reaction with their standard electrode potentials are : Pb(s)-2e^(-) rarr Pb^(2+)(aq) , E^(@)= - 0.30 V Ag(s) -e^(-) rarr Ag^(+) (aq), E^(@)= + 0.80 V Which of the following reaction takes place ?