The cell that will measure the standard electrode potential of a copper electrode is:

1. Pt(s) | H2(g, \(1 \over 10\) bar) | H+(aq, 1M) || Cu2+(aq, 1M) | Cu
2. Pt(s) | H2(g, 1 bar) | H+(aq, 1M) || Cu2+ (aq, 2M) | Cu
3. Pt(s) | H2(g, 1 bar) | H+(aq, 1M)|| Cu2+ (aq, 1M) | Cu
4. Pt(s) | H2(g, \(1 \over 10\) bar) | H+(aq, \(1 \over 10\)M) || Cu2+(aq, 1M) | Cu

Subtopic:  Electrolytic & Electrochemical Cell |
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The electrode potential for Mg electrode varies according to the equation

\(E_{Mg^{2+}/Mg}\ = \ E_{Mg^{2+}/Mg}^{o} \ - \ \frac{0.059}{2}log\frac{1}{[Mg^{2+}]}\)

The graph of EMg2+ / Mg vs log [Mg2+] among the following is:

1.    2.  
3.    4.  
Subtopic:  Nernst Equation |
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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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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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The incorrect statement about an inert electrode in a cell is:

1. It does not participate in the cell reaction.
2. It provides surface either for oxidation or for the reduction reaction.
3. It provides a surface for the conduction of electrons.
4. It provides a surface for redox reaction.

Subtopic:  Electrode & Electrode Potential |
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An electrochemical cell can behave like an electrolytic cell when -

1. Ecell = 0

2. Ecell > Eext

3. Eext > Ecell

4. Ecell = Eext

Subtopic:  Electrolytic & Electrochemical Cell |
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The incorrect statement about the solution of electrolytes is:

1. Conductivity of solution depends upon the size of ions.
2. Conductivity depends upon the viscosity of solution.
3. Conductivity does not depend upon the solvation of ions present in solution.
4. Conductivity of solution increases with temperature.
Subtopic:  Conductance & Conductivity |
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Using the data given below find out the strongest reducing agent.

ECr2O72-/Cr3+=1.33V  ;  ECl2/Cl-=1.36VEMn04-/Mn2+=1.51V    ;  ECr3+/Cr=-0.74V

1.  Cl-

2.  Cr

3.  Cr3+

4.  Mn2+

 

Subtopic:  Electrochemical Series |
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Using the data given below find out the strongest oxidizing agent.

ECr2O72-/Cr3+=1.33V  ;  ECl2/Cl-=1.36VEMn04-/Mn2+=1.51V    ;  ECr3+/Cr=-0.74V

1.  Cl-

2.  Mn2+

3.  MnO4-

4.  Cr3+

Subtopic:  Electrochemical Series |
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ECr2O72-/Cr3+=1.33V  ;  ECl2/Cl-=1.36VEMn04-/Mn2+=1.51V    ;  ECr3+/Cr=-0.74V

Using the data given above find out in which option the order of reducing power is correct.

1.  Cr3+ < Cl- < Mn2+ < Cr

2.  Mn2+ < Cl- < Cr3+ < Cr

3.  Cr3+ < Cl- < Cr2O72- < MnO4-

4.  Mn2+ < Cr3+ < Cl- < Cr

 

Subtopic:  Electrochemical Series |
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