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 |
75%
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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 |
60%
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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 |
72%
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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 |
63%
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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 |
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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 |
63%
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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 |
74%
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Using the data given below find out the strongest reducing agent.

1.  Cl-

2.  Cr

3.  Cr3+

4.  Mn2+

Subtopic:  Electrochemical Series |
55%
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Using the data given below find out the strongest oxidizing agent.

$$\mathrm{E_{Cr_{2} O_{7}^{2 -} / Cr^{3 +}}^{\ominus} = 1 . 33 V ; E_{Cl_{2} / Cl^{-}}^{\ominus} = 1 . 36 V \\ E_{Mn O_{4}^{-} / Mn^{2 +}}^{\ominus} = 1 . 51 V ; E_{Cr^{3 +} / Cr}^{\ominus} = - 0 . 74 V}$$

1. Cl
2. Mn2+
3. MnO4
4. Cr3+
Subtopic:  Electrochemical Series |
66%
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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%
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