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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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%
From NCERT
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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%
From NCERT
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The cell constant of a conductivity cell-

1. Changes with the change of electrolyte.
2. Changes with the change of concentration of electrolyte.
3. Changes with the temperature of the electrolyte.
4. Remains constant for a cell.

Subtopic:  Conductance & Conductivity |
 80%
From NCERT
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The correct statement about charging of the lead storage battery is:

1. PbSO4 anode is reduced to Pb.

2. PbSO4 cathode is reduced to Pb.

3. PbSO4 cathode is oxidised to Pb.

4. PbSO4 anode is oxidised to PbO2.

Subtopic:  Batteries & Salt Bridge |
From NCERT
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\(\Lambda _{m(NH_{4}OH)}^{o}\) is equal to -
1. \(\Lambda _{m(NH_{4}OH)}^{o} \ + \ \Lambda _{m(NH_{4}Cl)}^{o} \ - \ \Lambda _{m(HCl)}^{o}\)
2. \(\Lambda _{m(NH_{4}Cl)}^{o} \ + \ \Lambda _{m(NaOH)}^{o} \ - \ \Lambda _{m(NaCl)}^{o}\)
3. \(\Lambda _{m(NH_{4}Cl)}^{o} \ + \ \Lambda _{m(NaCl)}^{o} \ - \ \Lambda _{m(NaOH)}^{o}\)
4. \(\ \Lambda _{m(NaOH)}^{o} \ + \ \Lambda _{m(NaCl)}^{o}\ - \ \Lambda _{m(NH_{4}Cl)}^{o}\)

Subtopic:   Kohlrausch Law & Cell Constant |
 88%
From NCERT
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The half-cell reaction at the anode during the electrolysis of aqueous sodium chloride solution  is represented by : 

1. Na+(aq) + e- ⟶ Na(s) ; \(E_{cell}^{o} \ = \ -2.71 \ V \)

2. 2H2O(l) ⟶ O2(g) + 4H+(aq) + 4e; \(E_{cell}^{o} \) = 1.23 V

3. H+(aq) + e-\(\frac{1}{2}\)H2(g) ; \(E_{cell}^{o} \) = 0.00 V

4. Cl-(aq) ⟶ \(\frac{1}{2}\)Cl2(g) + e- ; \(E_{cell}^{o}\) 1.36 V

Subtopic:  Electrolytic & Electrochemical Cell |
 68%
From NCERT
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