- 1(current)
Q. No.Match the redox conversions in List-I with the corresponding number of Faradays required in List-II.
Choose the correct answer from the options given below:
| List-I (Redox Conversion) |
List-II (Number of Faraday required) |
||
| A. | 1 mol of H2O to O2 | I. | 3F |
| B. | 1 mol of \(MnO^-_4\) to \(Mn^{2+}\) | II. | 2F |
| C. | 1.5 mol of \(Ca\) from molten \(CaCl_2\) | III. | 1F |
| D. | 1 mol of FeO to Fe2O3 | IV. | 5F |
Choose the correct answer from the options given below:
| 1. | A - III, B - IV, C - I, D - II | 2. | A - II, B - III, C - I, D - IV |
| 3. | A - III, B - IV, C - II, D - I | 4. | A - II, B - IV, C - I, D - III |
Subtopic: Faraday’s Law of Electrolysis |
66%
Level 2: 60%+
NEET - 2024
Hints
Mass in grams of copper deposited by passing 9.6487 A current through a voltmeter containing copper sulphate for 100 seconds is(Given : Molar mass of Cu: \(63 g mol^{-1}\) F = 96487 C)
| 1. | 0.315 g | 2. | 31.5 g |
| 3. | 0.0315 g | 4. | 3.15 g |
Subtopic: Faraday’s Law of Electrolysis |
68%
Level 2: 60%+
NEET - 2024
Hints
Given below are two statements:
In the light of the above statements, choose the correct answer from the options given below:
1. Both Statement I and Statement II are true
2. Both Statement I and Statement II are false
3. Statement I is true but Statement II is false
4. Statement I is false but Statement II is true
| Statement I: | \(2 \mathrm{~F}\) electricity is required for the oxidation of 1 mole \(\mathrm{H}_2 \mathrm{O}\) to \(\mathrm{O}_2\). |
| Statement II: | To get \(40.0 \mathrm{~g}\) of Aluminium from molten \(\mathrm{Al}_2 \mathrm{O}_3\) required electricity is \(4.44 \mathrm{~F}\). |
In the light of the above statements, choose the correct answer from the options given below:
1. Both Statement I and Statement II are true
2. Both Statement I and Statement II are false
3. Statement I is true but Statement II is false
4. Statement I is false but Statement II is true
Subtopic: Faraday’s Law of Electrolysis |
63%
Level 2: 60%+
NEET - 2024
Hints
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 |
(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 |
59%
Level 3: 35%-60%
NEET - 2022
Hints
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 |
70%
Level 2: 60%+
NEET - 2020
Hints
- 1(current)
Q. No.
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