# Match List I with List II. List I (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 |
61%
From NCERT
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 |
64%
From NCERT
NEET - 2024
Hints

Given below are two statements:
 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 |
58%
From NCERT
NEET - 2024
Hints

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 mmol–1
3. 124 S cm2 mol–1
4. 124 S m2 mol–1
Subtopic:  Conductance & Conductivity |
From NCERT
NEET - 2023
Hints

The correct value of cell potential in volt for the reaction that occurs when the following two half cells are connected, is:
$$\mathrm{Fe}_{\text {(aq) }}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Fe}(\mathrm{s}), \mathrm{E}^{\circ}=-0.44 \mathrm{~V}$$
$$\mathrm{Cr}_2 \mathrm{O}_7^{2-}{ }_{\text {(aq) }}+14 \mathrm{H}^{+}+6 e^{-} \rightarrow 2 \mathrm{Cr}^{3+}+7 \mathrm{H}_2 \mathrm{O},$$
$$\mathrm{E}^{\circ}=+1.33 \mathrm{~V}$$
 1 +1.77 V 2 +2.65 V 3 +0.01 V 4 +0.89 V
Subtopic:  Electrode & Electrode Potential |
72%
From NCERT
NEET - 2023
Hints

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:
 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 $$Mg(OH)_2$$
Which of the above statements are correct?
1. (A) and (B) only
2. (A), (B), and (C) only
3. (B) and (C) only
4. (B) and (D) only
Subtopic:  Conductance & Conductivity |
55%
From NCERT
NEET - 2023
Hints

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 |
77%
From NCERT
NEET - 2023
Hints

Given below are two statements: one is labelled as Assertion (A) and the other is labelled as Reason (R):
 Assertion (A): In equation $$\Delta_{\mathrm{r}} \mathrm{G}=-\mathrm{nFE} _{\text {cell }},$$ value $$\mathrm{\Delta_rG }$$ depends on n. Reason (R): $$\mathrm{E_{cell} }$$ is an intensive property and  $$\mathrm{\Delta_rG }$$  is an extensive property.

In the light of the above statements choose the correct answer from the options given below:

 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 |
57%
From NCERT
NEET - 2023
Hints

Standard electrode potential for the cell with cell reaction
Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)
is 1.1 V. Calculate the standard Gibbs energy change for the cell reaction.
(Given F = 96487 C mol–1)
 1 –200.27 kJ mol–1 2 –212.27 kJ mol–1 3 –212.27 J mol–1 4 –200.27 J mol–1
Subtopic:  Relation between Emf, G, Kc & pH |
80%
From NCERT
NEET - 2022
To view explanation, please take trial in the course.
NEET 2025 - Target Batch
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To view explanation, please take trial in the course.
NEET 2025 - Target Batch

Two half cell reactions are given below:
\begin{aligned} &\mathrm{Co}^{3+}+e^{-} \rightarrow \mathrm{Co}^{2+}, \mathrm{E}_{\mathrm{Co}^{2+} / \mathrm{Co}^{3+}}^{\circ}=-1.81 \mathrm{~V} \\ &2 \mathrm{Al}^{3+}+6 e^{-} \rightarrow 2 \mathrm{Al}(\mathrm{s}), \mathrm{E}_{\mathrm{Al} / \mathrm{Al}^{3+}}^{\circ}=+1.66 \mathrm{~V} \end{aligned}
The standard EMF of a cell with feasible redox reaction will be:

 1 +7.09 V 2 +0.15 V 3 +3.47 V 4 –3.47 V
Subtopic:  Electrode & Electrode Potential |
66%
From NCERT
NEET - 2022
To view explanation, please take trial in the course.
NEET 2025 - Target Batch
Hints
To view explanation, please take trial in the course.
NEET 2025 - Target Batch