# 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 molar conductance of NaCl, HCI, and CH3COONa at infinite dilution are 126.45, 426.16, and 91.0 S cm mol–1 respectively. The molar conductance of CH3COOH at infinite dilution will be:

1. 698.28 S cm2 mol–1

2. 540.48 S cm2 mol–1

3. 201.28 S cm2 mol–1

4. 390.71 S cm2 mol–1

Subtopic:   Kohlrausch Law & Cell Constant |
82%
From NCERT
NEET - 2021
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The molar conductivity of 0.007 M acetic acid is 20 S cm2 mol–1. The dissociation constant of acetic acid is :

($$\mathrm{\Lambda_{H^{+}}^{o} \ = \ 350 \ S \ cm^{2} \ mol^{-1} }$$)
($$\mathrm{\mathrm{\Lambda_{CH_{3}COO^{-}}^{o} \ = \ 50 \ S \ cm^{2} \ mol^{-1} }}$$)

1. $1.75×{10}^{-5}$ mol L–1

2. $2.50×{10}^{-5}$ mol L–1

3. $1.75×{10}^{-4}$ mol L–1

4. $2.50×{10}^{-4}$ mol L–1

Subtopic:   Kohlrausch Law & Cell Constant |
56%
From NCERT
NEET - 2021
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On electrolysis of dilute sulphuric acid using Platinum (Pt) electrode, the product obtained at the anode will be:

1. Oxygen gas

2. ${\mathrm{H}}_{2}\mathrm{S}$ gas

3. ${\mathrm{SO}}_{2}$ gas

4. Hydrogen gas

Subtopic:  Electrolytic & Electrochemical Cell |
64%
From NCERT
NEET - 2020
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The number of Faradays (F) required to produce 20 g of calcium from molten CaCl2 (Atomic mass of Ca = 40 g mol–1) is:

1. 2

2. 3

3. 4

4. 1

Subtopic:  Faraday’s Law of Electrolysis |
67%
From NCERT
NEET - 2020
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Given below are half-cell reactions:
$$\mathrm{MnO}_{4}^{-}+8 \mathrm{H}^{+}+5 \mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}+4 \mathrm{H}_{2} \mathrm{O},$$
$$\mathrm{E}_{\mathrm{Mn}^{2+}}^{\circ} / \mathrm{MnO}_{4}^{-}=-1.510 \mathrm{~V}$$
$$\frac{1}{2} \mathrm{O}_{2}+2 \mathrm{H}^{+}+2 \mathrm{e}^{-} \rightarrow \mathrm{H}_{2} \mathrm{O},$$
$$\mathrm{E}_{\mathrm{O}_{2} / \mathrm{H}_{2} \mathrm{O}}^{\circ}=+1.223 \mathrm{~V}$$
Will the permanganate ion, $$\mathrm{MnO}_{4}^{-}$$ , liberate $$\mathrm{O}_{2}$$ from water in the presence of an acid?

1. No, because $$\mathrm{E}_{\text {cell }}^{\circ}=-2.733 \mathrm{~V}$$
2. Yes, because $$\mathrm{E}_{\text {cell }}^{\circ}=+0.287 \mathrm{~V}$$
3. No, because $$\mathrm{E}_{\text {cell }}^{\circ}=-0.287 \mathrm{~V}$$
4. Yes, because $$\mathrm{E}_{\text {cell }}^{\circ}=+2.733 \mathrm{~V}$$
Subtopic:  Electrode & Electrode Potential |
From NCERT
NEET - 2022
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Find the emf of the cell in which the following reaction takes place at 298 K:
$$\mathrm{Ni}(\mathrm{s})+2 \mathrm{Ag}^{+}(0.001 \mathrm{M}) \rightarrow \mathrm{Ni}^{2+}(0.001 \mathrm{M})+2 \mathrm{Ag}(\mathrm{s})$$
$$\small{\text { (Given that } \mathrm{E}_{\text {cell }}^{\circ}=10.5 \mathrm{~V}, \frac{2.303 \mathrm{RT}}{\mathrm{F}}=0.059 \text { at } \ 298 \mathrm{~K})}$$
1. 1.05 V
2. 1.0385 V
3. 1.385 V
4. 0.9615 V

Subtopic:  Nernst Equation |
From NCERT
NEET - 2022
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The three cells with their $$E^\circ_{\text{(cell)}}$$ values are given below:

 Cells $$E^\circ_{\text{(cell)}}/V$$ (a) Fe|Fe2+||Fe3+|Fe 0.404 (b) Fe|Fe2+||Fe3+, Fe2+|Pt 1.211 (c) Fe|Fe3+||Fe3+, Fe2+|Pt 0.807
The standard Gibbs free energy change values for three cells are, respectively:
(F represents the charge on 1 mole of electrons.)

 1 –1.212 F, –1.211 F, –0.807 F 2 +2.424 F, +2.422 F, +2.421 F 3 –0.808 F, –2.422 F, –2.421 F 4 –2.424 F, –2.422 F, –2.421 F
Subtopic:  Faraday’s Law of Electrolysis |
56%
From NCERT
NEET - 2022
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$$\land^o_m$$ for NaCl, HCl and $$\mathrm{CH_3COONa }$$ are 126.4, 425.9, and 91.05 S cm2 mol–1 respectively. If the conductivity of 0.001028 mol L–1 acetic acid solution is $$4.95 \times 10^{-5} S ~cm^{-1}$$, the degree of dissociation of the acetic acid solution is:

 1 0.01233 2 1 3 0.1233 4 1.233
Subtopic:  Conductance & Conductivity |
56%
From NCERT
NEET - 2022
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Two half cell reactions are given below:
\begin{aligned} &\mathrm{Co}^{3+}+e^{-} \rightarrow \mathrm{Co}^{2+}, \mathrm{E}_{\mathrm{Co}^{2+} / \mathrm{Co}^{3+}}^{\circ}=-1.81 \mathrm{~V} \\ &2 \mathrm{Al}^{3+}+6 e^{-} \rightarrow 2 \mathrm{Al}(\mathrm{s}), \mathrm{E}_{\mathrm{Al} / \mathrm{Al}^{3+}}^{\circ}=+1.66 \mathrm{~V} \end{aligned}
The standard EMF of a cell with feasible redox reaction will be:

 1 +7.09 V 2 +0.15 V 3 +3.47 V 4 –3.47 V
Subtopic:  Electrode & Electrode Potential |
66%
From NCERT
NEET - 2022
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