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Q. No.When \(CuSO_4\) solution is electrolysed using inert electrodes, the incorrect statement regarding this electrolysis is:
1.
weight of cathode increases
2.
pH of the solution remains unchanged
3.
product at the anode is \(O_2\) gas
4.
weight of the anode is unchanged
Subtopic: Electrolytic & Electrochemical Cell |
52%
From NCERT
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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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\(\land^o_m\) 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 |
59%
From NCERT
NEET - 2022
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For a given cell, a 0.1 molar solution has a resistance of \(20 \ \Omega\) and molar conductivity of \(0.154 \times 10^{-3} S~cm^2~mol^{-1} \).
The value of the cell constant is:
The value of the cell constant is:
| 1. | \(3.08 \times 10^{-7} cm^{-1}\) | 2. | \(30.8 \times 10^{-7} cm^{-1}\) |
| 3. | \(0.308 \times 10^{-9} cm^{-1}\) | 4. | \(4.08 \times 10^{-6} cm^{-1}\) |
Subtopic: Conductance & Conductivity |
77%
From NCERT
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What is the nearest integer value of \(x\) for the Gibbs free energy change at 298 K, expressed as \(x×10^{−1}~kJ mol^{−1}\) for the given reaction.
\(Cu(s)+Sn^{2+}(0.001 M)\rightarrow Cu^{2+}(0.01M)+Sn(s) \)
Given: \(\small{E^\ominus_{Cu^{2+}/Cu}=0.34~V;~E^\ominus_{Sn^{2+}/Sn}=-0.14~V;~F=96500~C~mol^{-1}}\)
1. 873
2. 983
3. 1002
4. 911
Subtopic: Relation between Emf, G, Kc & pH |
50%
From NCERT
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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 |
82%
From NCERT
NEET - 2022
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Consider the following reactions:
\(\mathrm{MnO}_4^{-}+\mathrm{e}^{-} \rightarrow \mathrm{MnO}_4^{2-} ; E^\circ=+0.56 \mathrm{~V} \\ \mathrm{F}_2+2 \mathrm{e}^{-} \rightarrow 2 \mathrm{~F}^{-} ; E^\circ=+2.87 \mathrm{~V} \\ \mathrm{Co}^{3+}+\mathrm{e}^{-} \rightarrow \mathrm{Co}^{2+} ; E^\circ=+1.81 \mathrm{~V} \\ \mathrm{V}^{3+}+\mathrm{e}^{-} \rightarrow \mathrm{V}^{2+} ; E^\circ=-0.26 \mathrm{~V}\)
Select the correct option for increasing the order of reducing power:
1. \(\mathrm{V}^{2+}<\mathrm{MnO}_4^{2-}<\mathrm{Co}^{2+}<\mathrm{F}^{-} \)
2. \(\mathrm{MnO}_4^{2-}<\mathrm{V}^{2+}<\mathrm{Co}^{2+}<\mathrm{F}^{-} \)
3. \(\mathrm{F}^{-}<\mathrm{Co}^{2+}<\mathrm{MnO}_4^{2-}<\mathrm{V}^{2+} \)
4. \(\mathrm{Co}^{2+}<\mathrm{F}^{-}<\mathrm{MnO}_4^{2-}<\mathrm{V}^{2+} \)
\(\mathrm{MnO}_4^{-}+\mathrm{e}^{-} \rightarrow \mathrm{MnO}_4^{2-} ; E^\circ=+0.56 \mathrm{~V} \\ \mathrm{F}_2+2 \mathrm{e}^{-} \rightarrow 2 \mathrm{~F}^{-} ; E^\circ=+2.87 \mathrm{~V} \\ \mathrm{Co}^{3+}+\mathrm{e}^{-} \rightarrow \mathrm{Co}^{2+} ; E^\circ=+1.81 \mathrm{~V} \\ \mathrm{V}^{3+}+\mathrm{e}^{-} \rightarrow \mathrm{V}^{2+} ; E^\circ=-0.26 \mathrm{~V}\)
Select the correct option for increasing the order of reducing power:
1. \(\mathrm{V}^{2+}<\mathrm{MnO}_4^{2-}<\mathrm{Co}^{2+}<\mathrm{F}^{-} \)
2. \(\mathrm{MnO}_4^{2-}<\mathrm{V}^{2+}<\mathrm{Co}^{2+}<\mathrm{F}^{-} \)
3. \(\mathrm{F}^{-}<\mathrm{Co}^{2+}<\mathrm{MnO}_4^{2-}<\mathrm{V}^{2+} \)
4. \(\mathrm{Co}^{2+}<\mathrm{F}^{-}<\mathrm{MnO}_4^{2-}<\mathrm{V}^{2+} \)
Subtopic: Electrochemical Series |
75%
From NCERT
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The molar conductance of acetic acid is \(40~ \text S~\text {cm}^2 ~\text {mol}^{-1} \). If the dissociation constant is \(1 \times 10^{-5} \), then the concentration of acetic acid is:
\(\left (\Lambda_{\mathrm{NaAc}}^o=90 \mathrm{~S} \mathrm{~cm}^2 / \mathrm{mol} ~,{\mathrm{\Lambda^o_{NaCl}}}=120 \mathrm{~S} \mathrm{~cm}^2 / \mathrm{mol}\right. \) and \(\wedge_{HCl}^{o} = 430 \ S \ cm^{2} \ mol^{-1}) \)
1. \(9 \times 10^{-4}~ \text {mol} ~\text L^{-1} \)
2. \(9 \times 10^{-3}~ \text {mol} ~\text L^{-1} \)
3. \(400 ~\text {Scm}^2 ~\text {mol}^{-1} \)
4. \(40 ~\text {Scm}^2 ~\text {mol}^{-1} \)
\(\left (\Lambda_{\mathrm{NaAc}}^o=90 \mathrm{~S} \mathrm{~cm}^2 / \mathrm{mol} ~,{\mathrm{\Lambda^o_{NaCl}}}=120 \mathrm{~S} \mathrm{~cm}^2 / \mathrm{mol}\right. \) and \(\wedge_{HCl}^{o} = 430 \ S \ cm^{2} \ mol^{-1}) \)
1. \(9 \times 10^{-4}~ \text {mol} ~\text L^{-1} \)
2. \(9 \times 10^{-3}~ \text {mol} ~\text L^{-1} \)
3. \(400 ~\text {Scm}^2 ~\text {mol}^{-1} \)
4. \(40 ~\text {Scm}^2 ~\text {mol}^{-1} \)
Subtopic: Conductance & Conductivity |
62%
From NCERT
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Dissociation constant of a weak acid (HA) in terms of \(\Lambda_{m}^{\infty} \) and \(\Lambda_{m}{}\) is:
1. \(K_{a}=\frac{C \Lambda_{m}^{\infty}}{\left(\Lambda_{m}-\Lambda^{\infty}\right)}\)
2. \(K_{a}=\frac{C \Lambda_{m}^{2}}{\Lambda_{m}^{\infty}\left(\Lambda_{m}^{\infty}-\Lambda_{m}\right)} \)
3. \(K_{a}=\frac{C\left(\Lambda_{m}^{\infty}\right)^{2}}{\Lambda_{m}^{\infty}\left(\Lambda_{m}^{\infty}-\Lambda_{m}\right)}\)
4. None of the above
1. \(K_{a}=\frac{C \Lambda_{m}^{\infty}}{\left(\Lambda_{m}-\Lambda^{\infty}\right)}\)
2. \(K_{a}=\frac{C \Lambda_{m}^{2}}{\Lambda_{m}^{\infty}\left(\Lambda_{m}^{\infty}-\Lambda_{m}\right)} \)
3. \(K_{a}=\frac{C\left(\Lambda_{m}^{\infty}\right)^{2}}{\Lambda_{m}^{\infty}\left(\Lambda_{m}^{\infty}-\Lambda_{m}\right)}\)
4. None of the above
Subtopic: Conductance & Conductivity |
75%
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| Statement I: | Corrosion of metals considered as an electrochemical phenomenon. |
| Statement II: | Mg and Zn can be used as sacrificial electrodes during the corrosion of iron the electrode. |
In light of the above statement, choose the correct option among the following:
| 1. | Statement I is correct but Statement II is incorrect. |
| 2. | Statement I is incorrect but Statement II is correct. |
| 3. | Both Statement I and Statement II are incorrect. |
| 4. | Both Statement I and Statement II are correct. |
Subtopic: Corrosion |
73%
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