# Standard electrode potential of three metals X, Y and Z are -1.2 V, +0.5 V and -3.0 V respectively. The reducing power of these metals will be:  1. Y > X > Z 2. Z > X > Y 3. X > Y > Z 4. Y > Z > X

Subtopic:  Electrode & Electrode Potential |
81%
From NCERT
AIPMT - 2011
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If the  ${E}_{cell}^{}$ $0$for a given reaction has a negative value, then which of the following gives the correct relationship for the values of $∆{G}^{0}$  $and$   ${K}_{eq}$?

1.  $∆{\mathrm{G}}^{0}<0;$ ${\mathrm{K}}_{\mathrm{eq}}>1$

2.  $∆{\mathrm{G}}^{0}<0;$ ${\mathrm{K}}_{\mathrm{eq}}<1$

3.  $∆{\mathrm{G}}^{0}>0;$ ${\mathrm{K}}_{\mathrm{eq}}<1$

4.  $∆{\mathrm{G}}^{0}>0;$ ${\mathrm{K}}_{\mathrm{eq}}>1$

Subtopic:  Electrolytic & Electrochemical Cell | Relation between Emf, G, Kc & pH |
78%
From NCERT
AIPMT - 2011
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Based on electrode potentials in the table below:
 Cu2+(aq) + e- → Cu+(aq) 0.15 V Cu+(aq) + e- → Cu(s) 0.50 V

The value of $$E_{Cu^{2+}/Cu}^{o}$$ will be:
 1 0.325 V 2 0650 V 3 0.150 V 4 0.500 V
Subtopic:  Electrode & Electrode Potential |
60%
From NCERT
AIPMT - 2011
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Standard electrode potential for Sn4+/Sn2+ couple is +0.15 V and that for Cr3+/Cr couple is -0.74. 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%
From NCERT
AIPMT - 2011
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In producing chlorine by electrolysis, 100 kW power at 125 V is being consumed.
How much chlorine per minute is liberated:
(Given -ECE of chlorine is 0.367 X 10-6 kgC-1)

1. $kg$

2. $9.67×{10}^{-3}$ $kg$

3. $17.61×{10}^{-3}$ $kg$

4. $3.67×{10}^{-3}$ $kg$

Subtopic:  Faraday’s Law of Electrolysis |
52%
From NCERT
AIPMT - 2010
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For the reduction of silver ions with copper metal, the standard cell potential was found to be +0.46 V at 25 °C. The value of standard Gibbs energy, ΔGo will be:

(F = 96500 C mol-1)

1. -89.0 kJ

2. -89.0 J

3. -44.5 kJ

4. -98.0 kJ

Subtopic:  Faraday’s Law of Electrolysis |
69%
From NCERT
AIPMT - 2010
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An increase in equivalent conductance of a strong electrolyte with dilution is mainly due to:

 1 increase in ionic mobility of ions 2 100% ionization of electrolyte at normal dilution 3 increase in both, i.e, number of ions and ionic mobility of ions 4 increase in the number of ions

Subtopic:  Conductance & Conductivity |
AIPMT - 2010
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Al2Ois reduced by electrolysis at low potentials and high currents. If 4.0 x 10A of current is passed through molten Al2O3 for 6 hours, the mass of aluminum produced is:
(Assume 100 % current efficiency, the atomic mass of Al = 27 g mol-1)

 1 9.0 x 103 g 2 8.1 x 104 g 3 2.4 x 105 g 4 1.3 x 104 g
Subtopic:  Faraday’s Law of Electrolysis |
65%
From NCERT
AIPMT - 2009
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The molar conductance of $\frac{\mathrm{M}}{32}$ solution of a weak monobasic acid is 8.0 ohm-1 cmand at infinite dilution is 400 ohm-1 cm2. The dissociation constant of this acid is:

 1 $$1.25 \times10^{-5}$$ 2 $$1.25 \times10^{-6}$$ 3 $$6.25 \times10^{-4}$$ 4 $$1.25 \times10^{-4}$$
Subtopic:   Kohlrausch Law & Cell Constant |
64%
From NCERT
AIPMT - 2009
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Given:
(i) ${\mathrm{Cu}}^{2+}+2{\mathrm{e}}^{-}\to \mathrm{Cu}$    Eo = 0.337 V
(ii) ${\mathrm{Cu}}^{2+}+{\mathrm{e}}^{-}\to {\mathrm{Cu}}^{+}$  Eo = 0.153 V
Electrode potential, Eo for the reaction,
${\mathrm{Cu}}^{+}+{\mathrm{e}}^{-}\to \mathrm{Cu}$, will be:

1. 0.52 V

2. 0.90 V

3. 0.30 V

4. 0.38 V

Subtopic:  Relation between Emf, G, Kc & pH |
75%
From NCERT
AIPMT - 2009
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