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Q. No.Match the redox conversions in List-I with the corresponding number of Faradays required in List-II.
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
(Redox Conversion)
(Number of Faraday required)
Subtopic: Faraday’s Law of Electrolysis |
66%
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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 |
68%
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NEET - 2024
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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 |
64%
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NEET - 2024
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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%
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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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NEET - 2024
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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 \(90 ~\text{S} ~\text{cm}^2 ~\text{mol}^{-1}\), its extent (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. \(0.125\)
1. \( 0.225 \)
2. \( 0.215 \)
3. \(0.115 \)
4. \(0.125\)
Subtopic: Conductance & Conductivity |
60%
From NCERT
NEET - 2025
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The molar conductance of a solution, given its conductivity (0.248 S m–1) and concentration (0.2 mol m–3) is:
| 1. | 0.124 S cm2 mol–1 | 2. | 1.24 S m2 mol–1 |
| 3. | 124 S cm2 mol–1 | 4. | 124 S m2 mol–1 |
Subtopic: Conductance & Conductivity |
From NCERT
NEET - 2023
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The correct value of cell potential in volts for the reaction that occurs when the following two half cells are connected, is:
\(\mathrm{{Fe}_{ {(aq) }}^{2+}+2 {e}^{-} \rightarrow {Fe}({s}), {E}^{\circ}=-0.44{~V} }\)
\( \mathrm{{Cr}_2 {O}_7^{2-}{ }_{ {(aq) }}+14 {H}^{+}+6 e^{-} \rightarrow 2 {Cr}^{3+}+7 {H}_2 {O}},\)
\( \mathrm{{E}^{\circ}=+1.33 {~V}}\)
1. +1.77 V
2. +2.65 V
3. +0.01 V
4. +0.89 V
\(\mathrm{{Fe}_{ {(aq) }}^{2+}+2 {e}^{-} \rightarrow {Fe}({s}), {E}^{\circ}=-0.44{~V} }\)
\( \mathrm{{Cr}_2 {O}_7^{2-}{ }_{ {(aq) }}+14 {H}^{+}+6 e^{-} \rightarrow 2 {Cr}^{3+}+7 {H}_2 {O}},\)
\( \mathrm{{E}^{\circ}=+1.33 {~V}}\)
1. +1.77 V
2. +2.65 V
3. +0.01 V
4. +0.89 V
Subtopic: Electrode & Electrode Potential |
74%
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NEET - 2023
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The molar conductance of an electrolyte increases with dilution according to the equation:
\(\Lambda_{\mathrm{m}}=\Lambda_{\mathrm{m}}^{\circ}-\mathrm{A} \sqrt{\mathrm{c}} \)
Consider the following four statements:
Which of the above statements are correct?
\(\Lambda_{\mathrm{m}}=\Lambda_{\mathrm{m}}^{\circ}-\mathrm{A} \sqrt{\mathrm{c}} \)
Consider the following four statements:
| A: | This equation applies to both strong and weak electrolytes. |
| B: | The value of the constant A depends upon the nature of the solvent. |
| C: | The value of constant A is the same for both \(BaCl_2\) and \(MgSO_4\) |
| D: | The value of constant A is the same for both \(BaCl_2\) and \(Mg(OH)_2\) |
| 1. | (A) and (B) only | 2. | (A), (B), and (C) only |
| 3. | (B) and (C) only | 4. | (B) and (D) only |
Subtopic: Conductance & Conductivity |
57%
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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 |
81%
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NEET - 2023
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