# 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%
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NEET - 2020
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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%
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NEET - 2020
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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%
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NEET - 2020
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Limiting molar conductivities, for the given solutions, are :

$mo{l}^{-1}$

$mo{l}^{-1}$

$mo{l}^{-1}$

From the data given above, it can be concluded that $$\lambda_m^0$$ in ($$S\ cm^2\ mol^{-1}$$) for CH3COOH will be :

 1 $$\mathrm{x-y+2z}$$ 2 $$\mathrm{x+y+z}$$ 3 $$\mathrm{x-y+z}$$ 4 $$\mathrm{{(x-y) \over 2}+z}$$
Subtopic:  Conductance & Conductivity |
69%
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NEET - 2019
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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 |
81%
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%
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NEET - 2021
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For a cell involving one electron  at 298 K.
The equilibrium constant for the cell reaction is :
$\left[\mathrm{Given}\right]$ $\mathrm{that}$ $\frac{2.303}{}$ $\mathrm{RT}\mathrm{F}=0.059$ $\mathrm{V}$ $\mathrm{at}$ $\mathrm{T}=298$ $\mathrm{K\right)}$

1. $1.0×{10}^{30}$

2. $1.0×{10}^{2}$

3. $1.0×{10}^{5}$

4. $1.0×{10}^{10}$

Subtopic:  Relation between Emf, G, Kc & pH |
69%
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NEET - 2019
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For the cell reaction $$2Fe^{3+}(aq) \ + \ 2I^{-}(aq)\rightarrow 2Fe^{2+}(aq) \ + \ I_{2}(aq)$$

$$E_{cell}^{o} \ = \ 0.24 \ V$$ at $298$ $\mathrm{K}$. The standard Gibbs energy ∆rG of the cell reaction is:

[Given:  $\mathrm{C}$ ${\mathrm{mol}}^{-1}$]

1. $23.16$ $\mathrm{kJ}$ ${\mathrm{mol}}^{-1}$

2. $-46.32$ $\mathrm{kJ}$ ${\mathrm{mol}}^{-1}$

3. $-23.16$ $\mathrm{kJ}$ ${\mathrm{mol}}^{-1}$

4. $46.32$ $\mathrm{kJ}$ ${\mathrm{mol}}^{-1}$

Subtopic:  Relation between Emf, G, Kc & pH |
74%
From NCERT
NEET - 2019
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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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