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Q. No.Calculate emf of the half cell given below :
Pt (s) | \(H_2\) (g, 2 atm) | HCl (aq, 0.02 M)
\(E^0_{H_2 / H^+}\) = 0 V
(Given : \(\frac{2.303 RT}{F} = 0.059\),
log 2 = 0.3010)
1. 0.109 V
2. 0.035 V
3. − 0.035 V
4. − 0.109 V
Pt (s) | \(H_2\) (g, 2 atm) | HCl (aq, 0.02 M)
\(E^0_{H_2 / H^+}\) = 0 V
(Given : \(\frac{2.303 RT}{F} = 0.059\),
log 2 = 0.3010)
1. 0.109 V
2. 0.035 V
3. − 0.035 V
4. − 0.109 V
Subtopic: Nernst Equation |
Level 3: 35%-60%
NEET - 2026
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A solution of copper sulphate is electrolysed for 10 minutes with a current of 1.5 amperes. The mass of copper deposited at cathode is:
(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
(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
Subtopic: Faraday’s Law of Electrolysis |
56%
Level 3: 35%-60%
NEET - 2026
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If the molar conductivity \(\left(\Lambda_{\mathrm{m}}\right)\) of a \(0.050 ~\text{mol}~ \text{L}^{-1}\) solution of a monobasic weak acid is \(90 ~\text{S} ~\text{cm}^2 ~\text{mol}^{-1}\), then its degree of dissociation will be: [Assume \(\Lambda_{+}^0=349.6~ \mathrm{S ~cm}^2 \mathrm{~mol}^{-1}\) and \(\mathrm{\Lambda}_{-}^{\circ}=50.4 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1} \)]
| 1. | \( 0.225 \) | 2. | \( 0.215 \) |
| 3. | \(0.115 \) | 4. | \(0.125\) |
Subtopic: Conductance & Conductivity |
59%
Level 3: 35%-60%
NEET - 2025
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Please attempt this question first.
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 |
65%
Level 2: 60%+
NEET - 2024
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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 |
67%
Level 2: 60%+
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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 |
62%
Level 2: 60%+
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From the following select the one which is not an example of corrosion:
| 1. | Rusting of an iron object |
| 2. | Production of hydrogen by electrolysis of water |
| 3. | Tarnishing of silver |
| 4. | Development of green coating on copper and bronze ornaments |
Subtopic: Corrosion |
83%
Level 1: 80%+
NEET - 2024
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The standard cell potential of the following cell \(\mathrm{{Zn}\left|{Zn}^{2+}({aq}) \| {Fe}^{2+}({aq})\right| {Fe}~\text{ is }~0.32 {~V}}.\) Calculate the standard Gibbs energy change for the reaction:
\(\mathrm{{Zn}({s})+{Fe}^{2+}({aq}) \rightarrow {Zn}^{2+}({aq})+{Fe}({s})}\)
(Given : \(1 \mathrm{~F}=96487 \mathrm{C} mol^{-1}\))
\(\mathrm{{Zn}({s})+{Fe}^{2+}({aq}) \rightarrow {Zn}^{2+}({aq})+{Fe}({s})}\)
(Given : \(1 \mathrm{~F}=96487 \mathrm{C} mol^{-1}\))
| 1. | \(-61.75 \mathrm{{~kJ} {~mol}}^{-1}\) | 2. | \(+5.006 \mathrm{{~kJ} {~mol}}^{-1}\) |
| 3. | \(-5.006 \mathrm{{~kJ} {~mol}}^{-1}\) | 4. | \(+61.75 \mathrm{{~kJ} {~mol}}^{-1}\) |
Subtopic: Relation between Emf, G, Kc & pH |
84%
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Given below are two statements:
| Assertion (A): | In the equation, \(\Delta_{\mathrm{r}} \mathrm{G}=-\mathrm{nFE} _{\text {cell }}, \) value of \(\mathrm{\Delta_rG }\) depends on n. |
| Reason (R): | \(\mathrm{E_{cell} }\) is an intensive property and \(\mathrm{\Delta_rG }\) is an extensive property. |
| 1. | (A) is False, but (R) is True. |
| 2. | Both (A) and (R) are True and (R) is the correct explanation of (A). |
| 3. | Both (A) and (R) are True and (R) is not the correct explanation of (A). |
| 4. | (A) is True, but (R) is False. |
Subtopic: Relation between Emf, G, Kc & pH |
58%
Level 3: 35%-60%
NEET - 2023
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The conductivity of centimolar solution of KCl at 25°C is 0.0210 ohm–1 cm–1 and the resistance of the cell containing the solution at 25°C is 60 ohm. The value of the cell constant is:
| 1. | 3.34 cm–1 | 2. | 1.34 cm–1 |
| 3. | 3.28 cm–1 | 4. | 1.26 cm–1 |
Subtopic: Conductance & Conductivity |
82%
Level 1: 80%+
NEET - 2023
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