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Q. No.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 volt 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 |
73%
From NCERT
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 |
55%
From NCERT
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 |
78%
From NCERT
NEET - 2023
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Given below are two statements: one is labelled as Assertion (A) and the other is labelled as Reason (R):
In the light of the above statements choose the correct answer from the options given below:
| 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. |
| 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%
From NCERT
NEET - 2023
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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)
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 |
81%
From NCERT
NEET - 2022
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NEET 2025 - Target Batch
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Two half cell reactions are given below:
\(\begin{aligned} &\mathrm{{Co}^{3+}+e^{-} \rightarrow {Co}^{2+}, {E}_{{Co}^{2+} / {Co}^{3+}}^{\circ}=-1.81 {~V}} \\ &2 \mathrm{{Al}^{3+}+6 e^{-} \rightarrow 2 {Al}({s}), {E}_{{Al} / {Al}^{3+}}^{\circ}=+1.66 {~V}} \end{aligned} \)
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 |
67%
From NCERT
NEET - 2022
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\(\land^o_m\) for NaCl, HCl and \(\mathrm{CH_3COONa }\) are 126.4, 425.9, and 91.05 S cm2 mol–1 respectively. If the conductivity of 0.001028 mol L–1 acetic acid solution is \(4.95 \times 10^{-5} S ~cm^{-1} \), the degree of dissociation of the acetic acid solution is:
| 1. | 0.01233 | 2. | 1.00 |
| 3. | 0.1233 | 4. | 1.233 |
Subtopic: Conductance & Conductivity |
58%
From NCERT
NEET - 2022
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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 |
57%
From NCERT
NEET - 2022
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Find the emf of the cell in which the following reaction takes place at 298 K:
\(\mathrm{Ni}(\mathrm{s})+2 \mathrm{Ag}^{+}(0.001 \mathrm{M}) \rightarrow \mathrm{Ni}^{2+}(0.001 \mathrm{M})+2 \mathrm{Ag}(\mathrm{s}) \)
\( \small{\text { (Given that } \mathrm{E}_{\text {cell }}^{\circ}=10.5 \mathrm{~V}, \frac{2.303 \mathrm{RT}}{\mathrm{F}}=0.059 \text { at } \ 298 \mathrm{~K})} \)
1. 1.05 V
2. 1.0385 V
3. 1.385 V
4. 0.9615 V
Subtopic: Nernst Equation |
From NCERT
NEET - 2022
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