The voltage of the cell given below increases with: 

Cell: Sn(s) + 2Ag+(aq) → Sn2+(aq) + 2Ag(s)

1. Increase in size of the silver rod.

2. Increase in the concentration of Sn2+ ions.

3. Increase in the concentration of Ag+ ions.

4. None of the above.

Subtopic:  Nernst Equation |
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EFe2+Fe = -0.441 V and EFe3+Fe2+ =0.771 V, the standard emf of the reaction

Fe + 2Fe3+          3Fe2+will be

1. 0.111V

2. 0.330V

3. 1.653V

4. 1.212V

Subtopic:  Electrode & Electrode Potential |
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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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If an iron rod is dipped in CuSO4 solution, then:

1. Blue colour of the solution turns red.

2. Brown layer is deposited on iron rod.

3. No change occurs in the colour of the solution.

4. None of the above.

Subtopic:  Electrochemical Series |
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Without losing it's concentration, ZnCl2 solution cannot be kept in contact with :

1. Au

2. Al

3. Pb

4. Ag

Subtopic:  Electrochemical Series |
 74%
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The standard reduction potential at 290 K for the following half reactions are,

(i) Zn2+ + 2e— → Zn(s);      E° = -0.762 V

(ii) Cr3+ + 3e → Cr(s);          E° = -0.740 V

(iii) 2H+ + 2e → H2(g); ·      E° = +0.000 V

(iv) Fe3+ + e → Fe2+;         E° = +0.77V

Which is the strongest reducing agent?

1. Zn

2. Cr

3. Fe2+

4. H2

Subtopic:  Electrode & Electrode Potential |
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Which graph correctly correlates Ecell as a function of concentrations for the cell (for different values of M and M') ?

Zn(s) + Cu2+(M)           Zn2+(M') + Cu(s);
                Ecell = 1.10 V
X-axis : log10Zn2+Cu2+, Y-axis : Ecell 

1.                         2. 
3.                         4. 

Subtopic:  Nernst Equation |
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The most convenient method to protect the bottom of the ship made of iron is 

1. coating it with red lead oxide

2. white tin plating 

3. connecting it with Mg block

4. connecting it with Pb block

Subtopic:  Corrosion |
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The electrode potentials for

      Cu2+(aq) + e-           Cu+(aq)
and Cu+(aq) + e-  Cu(s)          

are +0.15 V and +0.50 V respectively. The value of ECu2+Cu will be

1. 0.325 V

2. 0.650 V

3. 0.150 V

4. 0.500 V

Subtopic:  Relation between Emf, G, Kc & pH |
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The Zn acts as sacrificial or cathodic protection to prevent rusting of iron because:

1. EOP of Zn < EOP of Fe

2. EOP of Zn > EOP of Fe

3. EOP of Zn = EOP of fe

4. Zn is cheaper than iron

Subtopic:  Corrosion |
 75%
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