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Question

Given the standard half-cell potentials (Eo) of the following as

Zn=Zn2++2e; Eo=+0.76V
Fe=Fe2++2e; Eo=+0.41V
Then the standard e.m.f. of the cell with the reaction Fe2++ZnZn2++Fe is?

  1. 0.35V
  2. +0.35V
  3. +1.17V
  4. 1.17V

A
0.35V
B
1.17V
C
+0.35V
D
+1.17V
Solution
Verified by Toppr

Zn+2+2eZn ; Eo=0.76 V (SRP) (Anode)

Fe+2+2eFe ; Eo=0.41 V (SRP) (Cathode)

Eocell=E+Fe+2/FeEoZn+2/Zn

=0.41+0.76=0.35V.

Hence, the correct option is B

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Similar Questions
Q1
Given the standard half-cell potentials (Eo) of the following as

Zn=Zn2++2e; Eo=+0.76V
Fe=Fe2++2e; Eo=+0.41V
Then the standard e.m.f. of the cell with the reaction Fe2++ZnZn2++Fe is?

View Solution
Q2
The standard reduction potential Eo for the half reactions are as
ZnZn2++2e; Eo=+0.76V
FeFe2++2e; Eo=+0.41V
The emf for cell reaction,
Fe2++ZnZn2++Fe, is
View Solution
Q3
The standard reduction potential Eo for half reactions are,

ZnZn2++2e;Eo=0.76 V

Fe2++2eFe;Eo=+0.41 V

The emf of the cell reaction; Fe2++ZnZn2++Fe is:

View Solution
Q4
The standard oxidation potentials Eo, for the half cell reactions are given as
ZnZn2++2e, E=+0.76 VFeFe2++2e, E=+0.41 V
The EMF for the cell reaction,
Fe2++ZnZn2++Fe is:
View Solution
Q5
The standard reduction potential Eo for half reaction are:

ZnZn2++2e;Eo=+0.76V
FeFe2++2e;Eo=+0.41V

The EMF of the cell reaction is:
Fe2++ZnZn2++Fe

View Solution