# At 25 ºC molar conductance of 0.1 molar aqueous solution of ammonium hydroxide is 9.54 ohm–1cm2 mol–1 and at infinite dilution, its molar conductance is 238 ohm–1 cm2 mol–1. The degree of ionization of ammonium hydroxide at the same concentration and temperature are: 1. 20.800% 2. 4.008% 3. 40.800% 4. 2.080%

Subtopic:   Kohlrausch Law & Cell Constant |
82%
From NCERT
AIPMT - 2013
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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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Limiting molar conductivity of NH4OH (i.e., ${\mathrm{\Lambda }}_{\mathrm{m}\left({\mathrm{NH}}_{4}\mathrm{OH}\right)}^{0}$ is equal to -

1. ${\mathrm{\Lambda }}_{\mathrm{m}\left(\mathrm{NaOH}\right)}^{0}+{\mathrm{\Lambda }}_{\mathrm{m}\left(\mathrm{NaCl}\right)}^{0}-{\mathrm{\Lambda }}_{\mathrm{m}\left(\mathrm{NaOH}\right)}^{0}$

2. ${\mathrm{\Lambda }}_{\mathrm{m}\left(\mathrm{NaOH}\right)}^{0}+{\mathrm{\Lambda }}_{\mathrm{m}\left(\mathrm{NaCl}\right)}^{0}-{\mathrm{\Lambda }}_{\mathrm{m}\left({\mathrm{NH}}_{4}\mathrm{Cl}\right)}^{0}$

3. ${\mathrm{\Lambda }}_{\mathrm{m}\left({\mathrm{NH}}_{4}\mathrm{OH}\right)}^{0}+{\mathrm{\Lambda }}_{\mathrm{m}\left({\mathrm{NH}}_{4}\mathrm{Cl}\right)}^{0}-{\mathrm{\Lambda }}_{\mathrm{m}\left(HCl\right)}^{0}$

4. ${\mathrm{\Lambda }}_{\mathrm{m}\left({\mathrm{NH}}_{4}\mathrm{Cl}\right)}^{0}+{\mathrm{\Lambda }}_{\mathrm{m}\left(\mathrm{NaOH}\right)}^{0}-{\mathrm{\Lambda }}_{\mathrm{m}\left(\mathrm{NaCl}\right)}^{0}$

Subtopic:   Kohlrausch Law & Cell Constant |
90%
From NCERT
AIPMT - 2012
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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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