Q. No.(Given : Molar mass of Cu = 63 g mol-1; 1 F = 96487 C mol-1)
1. 2.4036 g
2. 1.7018 g
3. 0.5876 g
4. 0.2938 g
| 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 |
(Given : Molar mass of Cu: \(63~ g mol^{-1}\); 1F = 96487 C)
| 1. | 0.315 g | 2. | 31.5 g |
| 3. | 0.0315 g | 4. | 3.15 g |
| 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
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 |
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
During the electrolysis of molten sodium chloride, the time required to produce 0.10 mol of chlorine gas using a current of 3 amperes is:
1. 55 minutes
2. 110 minutes
3. 220 minutes
4. 330 minutes
The number of electrons delivered at the cathode during electrolysis by a current of 1 ampere in 60 seconds is:
(Given: Charge on electron = 1.60 × 10–19 C)
1.
2.
3.
4.
When 0.1 mol MnO42– is oxidized, the quantity of electricity required to completely oxidise MnO42– to MnO4– is:
| 1. | 96500 C | 2. | 2 × 96500 C |
| 3. | 9650 C | 4. | 96.50 C |
Calculate the mass of silver (atomic mass = 108) deposited by the same quantity of electricity that
liberates 5600 mL of O₂ at STP.
1. 5.4 g
2. 10.8 g
3. 54.0 g
4. 108.0 g
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