- 1(current)
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
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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Consider the following Galvanic cell.
By what value the cell voltage change when concentration of ions in anodic and cathodic compartments both increased by a factor of 10 at 298
1. +0.0591
2. -0.0591
3. -0.1182
4. 0
Subtopic: Electrode & Electrode Potential |
Level 4: Below 35%
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Hints
Given below are some reactions. The reaction which is not feasible is
1. \(2KClO_3 + I_2 \rightarrow 2KIO_3 + Cl_2 \uparrow\)
2. \(2KCl + I_2 \rightarrow 2KI + Cl_2 \uparrow\)
3. Both 1 and 2 are not feasible
4. \(2KI + Cl_2 \rightarrow 2KCl + I_2\)
1. \(2KClO_3 + I_2 \rightarrow 2KIO_3 + Cl_2 \uparrow\)
2. \(2KCl + I_2 \rightarrow 2KI + Cl_2 \uparrow\)
3. Both 1 and 2 are not feasible
4. \(2KI + Cl_2 \rightarrow 2KCl + I_2\)
Subtopic: Electrochemical Series | Electrode & Electrode Potential |
Level 4: Below 35%
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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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Subtopic: Electrode & Electrode Potential |
57%
Level 3: 35%-60%
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Given below are the half-cell reactions :
The Eº for 3Mn2+ → Mn + 2Mn3+ will be :
1. – 2.69 V; the reaction will occur
2. – 0.33 V; the reaction will not occur
3. – 0.33 V; the reaction will occur
4. – 2.69 V; the reaction will not occur
Subtopic: Electrode & Electrode Potential |
59%
Level 3: 35%-60%
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Q. No.
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