Consider the change in oxidation state of Bromine corresponding to different emf values as shown in the diagram below: 
 
Then the species undergoing disproportionation is:-

1. 

2. 

3. 

4. HBrO

Subtopic:  Electrode & Electrode Potential |
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In the electrochemical cell: 
  Zn | ZnSO4 (0.01 M) || CuSO4(1.0 M) | Cu, 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, \(\frac{RT}{F}\) = 0.059)

1. E1<E2

2. E1>E2

3. E2=0E1

4. E1=E2

Subtopic:  Electrode & Electrode Potential | Nernst Equation |
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A button cell used in watches functions as following 
Zn(s) + Ag2O(s) + H2O(l) \(\rightleftharpoons\) 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

Subtopic:  Electrode & Electrode Potential |
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Standard electrode potential of three metals X, Y and Z are -1.2 V, +0.5 V and -3.0 V respectively. The reducing power of these metals will be : 

1.  Y > X > Z

2.  Z > X > Y

3.  X > Y > Z

4.  Y > Z > X

Subtopic:  Electrode & Electrode Potential |
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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 \(E_{Cu^{2+}/Cu}^{o}\) will be:
1. 0.325 V
2. 0650 V
3. 0.150 V
4. 0.500 V

 
Subtopic:  Electrode & Electrode Potential |
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Standard electrode potential for Sn4+/Sn2+ couple is +0.15 V and that for Cr3+/Cr couple is -0.74. These two couples in their standard state are connected to make a cell. The cell potential will be:

1. +0.89 V

2. +0.18 V

3. +1.83 V

4. +1.199 V

Subtopic:  Electrode & Electrode Potential |
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Consider the following relations for emf of an electrochemical cell:

(a) emf of cell = (Oxidation potential of anode) – (Reduction potential of cathode)
(b) emf of cell = (Oxidation potential of anode) + (Reduction potential of cathode)
(c) emf of cell = (Reduction potential of anode) + (Reduction potential of cathode)
(d) emf of cell = (Oxidation potential of anode) – (Oxidation potential of cathode)

The correct relation among the given options is : 

1. (a) and (b)

2. (c) and (d)

3. (b) and (d)

4. (c) and (a)

Subtopic:  Electrode & Electrode Potential |
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If EFe2+/Feo = -0.441 V and  EFe3+/Fe2+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

Subtopic:  Electrode & Electrode Potential |
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On the basis of the information available from the reaction :

43Al+O223Al2O3, G=-827 KJ mol-1

The minimum e.m.f. required to carry out electrolysis of Al2O3 is :
(F = 96500 C mol–1)

1. 2.14 V

2. 4.28 V

3. 6.42 V

4. 8.56 V

Subtopic:  Electrode & Electrode Potential |
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The EMF of a Daniel cell at 298 K is E Zn|ZnSO4(0.01 M) || CuSO4(1.0 M)|Cu .
When the concentration of ZnSO4 is 1.0 M and that of CuSO4 is 0.01 M, the EMF is changed to E2. The correct relationship between E1 and E2 is :

1. E1 > E2

2. E1 < E2

3. E1 = E2

4. E2 = 0 ≠ E1

Subtopic:  Electrode & Electrode Potential |
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