In a typical fuel cell, the reactants (R) and products (P) are: 

1. R = H2(g), O2(g); P = H2O2(l)
2. R = H2(g), O2(g); P = H2O(l)
3. R = H2(g) , O2(g) , C l2(g) ;   P = HClO4(aq)
4. R = H2(g) , N2(g) ;  P = NH3(aq)

Subtopic:  Batteries & Salt Bridge |
 73%
From NCERT
NEET - 2020
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The Gibb's energy for the decomposition of Al2O3 at 500°C is as follows: 

2/3Al2O3 → 4/3Al + O2 ; ∆rG = + 960 k J mol-1

The potential difference needed for the electrolytic reduction of aluminium oxide (Al2O3) at 500°C is at least,

1. 3.0 V 

2. 2.5 V 

3. 5.0 V 

4. 4.5 V 

Subtopic:  Relation between Emf, G, Kc & pH |
 60%
From NCERT
AIPMT - 2012
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Molar conductivities (°m) at infinite dilution of
NaCl, HCl, and CH3COONa are 126.4, 425.9, and 91.0 S cm2 mol-1 respectively.
 (°m)  for CH3COOH  will be: 

1. \(180.5~S~cm^2~mol^{-1}\) 2. \(290.8~S~cm^2~mol^{-1}\)
3. \(390.5~S~cm^2~mol^{-1}\) 4. \(425.5~S~cm^2~mol^{-1}\)
Subtopic:   Kohlrausch Law & Cell Constant |
 91%
From NCERT
AIPMT - 2012
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The correct expression that  represents the equivalent conductance at infinite dilution of Al2(SO4)3 is:

(Given that Al3+° and SO42-° are the equivalent conductances at infinite dilution of the respective ions)

1. Al3+° + SO42-°

2. Al3+° + SO42-°×6

3. 13Al3+° +12 SO42-°

4. 2Al3+° +3 SO42-°

Subtopic:  Conductance & Conductivity |
 59%
AIPMT - 2010
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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%
From NCERT
AIPMT - 2010
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105 coloumb charge liberated 1 gm silver (Ag). If the charge is doubled
then the amount of liberated Ag will be:

1. 1 gm 2. 2 gm
3. 3 gm 4. 4 gm
Subtopic:  Faraday’s Law of Electrolysis |
 86%
From NCERT
AIPMT - 1998
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The concentration of ZnCl2 solution will change when it is placed in a container which is made of:

1. Al 2. Cu
3. Ag 4. None
Subtopic:  Electrochemical Series |
 72%
From NCERT
AIPMT - 1998
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The cell reaction of an electrochemical cell is \(Cu^{2+}(C_{1}) + Zn \to Cu + Zn^{2+}(C_{2})\).

The change in free energy will be the function of:

\(1. \ ln (C_{1}+C_{2})\)
2. \(ln (\frac{C_{2}}{C_{1}})\)
\(3. \ ln C_{2}\)
\(4. \ lnC_{1}\)

Subtopic:  Relation between Emf, G, Kc & pH |
 93%
From NCERT
AIPMT - 1998
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4.5 g of aluminium (at. mass = 27 amu) is deposited at cathode from Al3+ solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from H+ ions in solution by the same quantity of electric charge will be:

1. 44.8 L 2. 11.2 L
3. 22.4 L 4. 5.6 L
Subtopic:  Faraday’s Law of Electrolysis |
 52%
From NCERT
AIPMT - 2005
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For the disproportionation of copper:

2Cu+ → C u2+ + C u, E° is:
(Given E° for Cu+2/Cu is 0.34 V & Eº for Cu+2/Cuis 0.15 V )

1. 0.49 V

2. – 0.19 V

3. 0.38 V

4. – 0.38 V

Subtopic:  Electrode & Electrode Potential |
From NCERT
AIPMT - 2000
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