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 |
 63%
From NCERT
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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 a 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 |
From NCERT
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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 |
 62%
From NCERT
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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 |
 73%
From NCERT
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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 |
 53%
From NCERT
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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 |
 63%
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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 |
 77%
From NCERT
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ECr2O72-/Cr3+=1.33V  ;  ECl2/Cl-=1.36VEMnO4-/Mn2+=1.51V    ;  ECr3+/Cr=-0.74V

Use the data given above to find out the most stable ion in its reduced form.

1. Cl-  2. Cr3+ 
3. Cr 4. Mn2+ 
Subtopic:  Electrochemical Series |
 65%
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The most stable oxidized species among the following is: 
\(E_{{\mathrm{Cr}_2 \mathrm{O}_7^2}/ \mathrm{Cr}^{3+}}^{o} =1.33 \mathrm{~V} ; E_{\mathrm{Cl}_2 / \mathrm{Cl}^{-}}^{o}=1.36 \mathrm{~V} \)
\( E_{\mathrm{MnO_{4}}^{-} / \mathrm{Mn}^{2+}}^{o}=1.51 \mathrm{~V} ; E_{\mathrm{Cr}^{3+} / \mathrm{Cr}}^{o}=-0.74 \mathrm{~V}\)

1. Cr3+  2. MnO4-
3. Cr2O72- 4. Mn2+ 
Subtopic:  Electrochemical Series |
 59%
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The quantity of charge required to obtain one mole of aluminium from Al2O3 is :

1.  1 F

2.  6 F

3.  3 F

4.  2 F

Subtopic:  Faraday’s Law of Electrolysis |
 67%
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