Electrode Electrode Potential

If ${\mathrm{E}}_{{\mathrm{Fe}}^{2+}/\mathrm{Fe}}^{\mathrm{o}}$ = -0.441 V and ${\mathrm{E}}_{{\mathrm{Fe}}^{3+}/{\mathrm{Fe}}^{2+}}^{\mathrm{o}}$ = 0.771 V, the standard emf of the reaction:

Fe + 2Fe³⁺→ 3Fe²⁺ will be:

1.	0.330 V	2.	1.653 V
3.	1.212 V	4.	0.111 V

Based on electrode potentials in the table below:

Cu2+(aq) + e- → Cu+(aq)	0.15 V
Cu+(aq) + e- → Cu(s)	0.50 V

The value of will be:

1.	0.325 V	2.	0650 V
3.	0.150 V	4.	0.500 V

What is the standard cell potential when the Sn⁴⁺/Sn²⁺ (E° = +0.15 V) and Cr³⁺/Cr (E° = −0.74 V) half-cells are connected under standard conditions?

1. +0.89 V

2. +0.18 V

3. +1.83 V

4. +1.199 V

A button cell used in watches functions as following
Zn(s) + Ag₂O(s) + H₂O(l) 2Ag(s) + Zn²⁺(aq) + 2OH^–(aq)
If half-cell potentials are-

Zn2+(aq) + 2e–→ Zn(s)	Eo = – 0.76 V
Ag2O(s) + H2O(l) + 2e– → 2Ag(s) + 2OH–(aq)	Eo = 0.34 V

The cell potential will be:

1.	0.42 V	2.	0.84 V
3.	1.34 V	4.	1.10 V

Consider the given cell:
$$
In the electrochemical cell, the emf of this Daniel cell is E₁. When the concentration of ZnSO₄ is changed to 1.0 M and that of CuSO₄ is changed to 0.01 M, the emf changes to E₂. From the following, which one is the relationship between E₁ and E₂ ?

(Given: = 0.059)

1.		2.
3.		4.

Consider the change in oxidation state of bromine corresponding to different emf values as shown in the diagram below: 


The species undergoing disproportionation is:

1.		2.
3.		4.

Given below are half-cell reactions:




Will the permanganate ion, , liberate from water in the presence of an acid?

1. No, because
2. Yes, because
3. No, because
4. Yes, because