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Q. No.A solution containing one mole per litre of each \(Cu(NO_3)_2; AgNO_3; Hg_2(NO_3)_2\) is being
electrolysed by using inert electrodes. The values of standard electrode potentials in volts
(reduction potentials) are:
\(\begin{aligned} & \mathrm{Ag} / \mathrm{Ag}^{+}=+0.80,2 \mathrm{Hg} / \mathrm{Hg}_2^{++}=+0.79 \\ & \mathrm{Cu} / \mathrm{Cu}^{++}=+0.34, \mathrm{Mg} / \mathrm{Mg}^{++}=-2.37 \end{aligned}\)
With increasing voltage, the sequence of deposition of metals on the cathode will be :
1. Ag, Hg, Cu, Mg
2. Mg, Cu, Hg, Ag
3. Ag, Hg, Cu
4. Cu, Hg, Ag
Subtopic: Electrode & Electrode Potential |
Level 4: Below 35%
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The standard reduction potentials of \(\mathrm{Cu}^{2+} \mid \mathrm{Cu} \text { and } \mathrm{Cu}^{2+} \mid \mathrm{Cu}^{+}\) are 0.337 V and 0.153V respectively. The standard electrode potential of Cu+|Cu half cell is:
1. 0.184 V
2. 0.827 V
3. 0.521 V
4. 0.490 V
1. 0.184 V
2. 0.827 V
3. 0.521 V
4. 0.490 V
Subtopic: Electrolytic & Electrochemical Cell |
Level 3: 35%-60%
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Identify the correct statement:
| 1. | The corrosion of iron can be minimised by forming contact with another metal with a higher reduction potential. |
| 2. | Iron corrodes in oxygen-free water |
| 3. | The corrosion of iron can be minimised by forming an impermeable barrier |
| 4. | Iron corrodes more rapidly in salt water because its electrochemical potential is higher. |
Subtopic: Corrosion |
Level 3: 35%-60%
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An aqueous solution of X is added slowly to an aqueous solution of Y as shown in List I. The variation in conductivity of these mixtures is given in List II. Match List I with List II and select the correct answer using the codes given below the table:
Codes:
| List-I | List-II | ||
| (P) |  |
(i) | Conductivity decreases and then increases. |
| (Q) |  |
(ii) | Conductivity decreases and then does not change much. |
| (R) |  |
(iii) | Conductivity increases and then does not change much. |
| (S) |  |
(iv) | Conductivity does not change much and then increases. |
Codes:
| P | Q | R | S | |
| 1. | (iii) | (iv) | (ii) | (i) |
| 2. | (iv) | (iii) | (ii) | (i) |
| 3. | (ii) | (iii) | (iv) | (i) |
| 4. | (i) | (iv) | (iii) | (ii) |
Subtopic: Conductance & Conductivity |
Level 3: 35%-60%
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| Half-Reaction | \(E^o(V)\) |
| \(2H^+ + 2e^- \rightarrow H_2\) | 0.00 |
| \(Pd^{2+} + 2e^- \rightarrow Pd\) | 0.90 |
| \(O_2 + 4H^+ + 4e^- \rightarrow 2H_2O\) | 1.23 |
According to the equations and data in the table above, which species is the strongest reducing agent of the following choices?
1. H+
2. H2
3. H2O
4. Pd2+
Subtopic: Electrode & Electrode Potential |
58%
Level 3: 35%-60%
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Extraction of chlorine from brine occurs when:
| 1. | \(\Delta G_V\) for the overall reaction is negative and EV for overall reaction has negative value. |
| 2. | \(\Delta G_V\) for the overall reaction is positive and EV for overall reaction has negative value. |
| 3. | \(\Delta G_V\) for the overall reaction is positive and EV for overall reaction has positive value. |
| 4. | \(\Delta G_V\) for the overall reaction is negative and EV for overall reaction has positive value. |
Subtopic: Relation between Emf, G, Kc & pH |
72%
Level 2: 60%+
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Subtopic: Electrode & Electrode Potential |
57%
Level 3: 35%-60%
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The Incorrect statement about the conductivity of electrolytic (ionic) solutions is:
| 1. | It is independent of the solvent viscosity |
| 2. | It depends on the size of the ions and their solvation |
| 3. | It increases with the increase in electrolyte concentration |
| 4. | It increases with the increase in temperature |
Subtopic: Conductance & Conductivity |
62%
Level 2: 60%+
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Given below are two statements:
| Assertion (A): | Molar conductivity increases with a decrease in concentration. |
| Reason (R): | For strong electrolytes, \(Λ_m\) increases slowly with dilution and can be represented by the equation: \(\Lambda_m=\Lambda_m^0-A c^{1 / 2}\) |
| 1. | Both (A) and (R) are True and (R) is the correct explanation of (A). |
| 2. | Both (A) and (R) are True but (R) is not the correct explanation of (A). |
| 3. | (A) is True but (R) is False. |
| 4. | Both (A) and (R) are False. |
Subtopic: Conductance & Conductivity |
51%
Level 3: 35%-60%
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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 |
56%
Level 3: 35%-60%
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