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 |
90%
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A button cell used in watches functions as following
Zn(s) + Ag2O(s) + H2O(l) $$\rightleftharpoons$$ 2Ag(s) + Zn2+(aq) + 2OH(aq)
If half-cell potentials are-

 Zn2+(aq) + 2e–→ Zn(s) Eo = – 0.76 V Ag2O(s) + H2O(l) + 2e– → 2Ag(s) + 2OH–(aq) Eo = 0.34 V

The cell potential will be:

 1 0.42 V 2 0.84 V 3 1.34 V 4 1.10 V
Subtopic:  Electrode & Electrode Potential |
86%
From NCERT
AIPMT - 2013
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The correct increasing order of reducing power of the metals is:

 K+/K = –2.93 V Ag+/Ag = 0.80 V Hg2+/Hg = 0.79 V Mg2+/Mg = –2.37 V Cr3+/Cr = – 0.74 V

 1 Cr

Subtopic:  Electrode & Electrode Potential |
85%
From NCERT
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Molten sodium chloride conducts electricity due to the presence of:

1. Free ions.

2. Free molecules.

3. Free electrons.

4. Atoms of sodium and chlorine.

Subtopic:  Electrode & Electrode Potential |
79%
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The metal that cannot be produced upon reduction of its oxide by aluminium is :

 1 K 2 Mn 3 Cr 4 Fe
Subtopic:  Electrode & Electrode Potential |
73%
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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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A gas X at 1 atm is bubbled through a solution containing a mixture of 1 M Yand 1 M Z- at 25 oC . If the reduction potential of Z > Y > X, then:

 1 Y will oxidize X but not Z. 2 Y will oxidize Z but not X. 3 Y will oxidize both X and Z. 4 Y will reduce both X and Z.

Subtopic:  Electrode & Electrode Potential |
68%
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If ${\mathrm{E}}_{{\mathrm{Fe}}^{2+}/\mathrm{Fe}}^{\mathrm{o}}$ = -0.441 V and  ${\mathrm{E}}_{{\mathrm{Fe}}^{3+}/{\mathrm{Fe}}^{2+}}^{\mathrm{o}}$ = 0.771 V, the standard emf of the reaction:

Fe + 2Fe3+→ 3Fe2+ will be:

 1 0.330 V 2 1.653 V 3 1.212 V 4 0.111 V
Subtopic:  Electrode & Electrode Potential |
71%
From NCERT
AIPMT - 2006
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Consider the following relations for emf of an electrochemical cell:

 (a) emf of cell = (Oxidation potential of anode) – (Reduction potential of cathode) (b) emf of cell = (Oxidation potential of anode) + (Reduction potential of cathode) (c) emf of cell = (Reduction potential of anode) + (Reduction potential of cathode) (d) emf of cell = (Oxidation potential of anode) – (Oxidation potential of cathode)

The correct relation among the given options is:

 1 (a) and (b) 2 (c) and (d) 3 (b) and (d) 4 (c) and (a)
Subtopic:  Electrode & Electrode Potential |
68%
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AIPMT - 2010
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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%
From NCERT
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