The standard electrode potential for Sn4+/Sn2+ couple is +0.15 V and that for the Cr3+/Cr couple is -0.74 V. 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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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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The correct increasing order of reducing the power of the metals is:

K+/K = –2.93 V
Ag+/Ag = 0.80 V
Hg2+/Hg = 0.79 V
Mg2+/Mg = –2.37 V
Cr3+/Cr = – 0.74 V

1. Cr < Mg < K < Ag < Hg

2. Mg < K < Ag < Hg < Cr

3. K < Ag < Hg < Cr < Mg

4. Ag < Hg < Cr < Mg < K

Subtopic:  Electrode & Electrode Potential |
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Molten sodium chloride conducts electricity due to the presence of : 

1. Free ions.

2. Free molecules.

3. Free electrons.

4. Atoms of sodium and chlorine.

Subtopic:  Electrode & Electrode Potential |
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The metal that cannot be produced upon reduction of its oxide by aluminium is :

1. K                                                        

2. Mn

3. Cr                                                      

4. Fe

Subtopic:  Electrode & Electrode Potential |
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The difference between the electrode potentials of two electrodes when no current is drawn through the cell is called : 

1. Cell potential.

2. Cell emf.

3. Potential difference.

4. Cell voltage.

Subtopic:  Electrode & Electrode Potential |
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A gas X at 1 atm is bubbled through a solution containing a mixture of 1 M Yand 1 M Z- at 25 oC . If the reduction potential of Z > Y > X, then : 
1. Y will oxidize X but not Z 
2. Y will oxidize Z but not X
3. Y will oxidize both X and Z 
4. Y will reduce both X and Z

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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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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The correct statement among the following options is: 

1. Ecell and ∆rG of cell reaction are both extensive properties.
2. Ecell and ∆rG of cell reaction are both intensive properties.
3. Ecell is an intensive property while ∆rG of cell reaction is an extensive property.
4. Ecell is an extensive property while ∆rG of cell reaction is an intensive property.

Subtopic:  Electrode & Electrode Potential |
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