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Q. No.The standard reduction potential of Zn2+/Zn and Cu2+/Cu is -0.76 and +0.34 V respectively. The oxidising agent and reducing agent, respectively, are
1.
Cu & Zn2+
2.
Zn & Cu
3.
Cu2+ & Zn2+
4.
Cu2+ & Zn
Subtopic: Electrochemical Series |
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Aqueous NaCl solution is electrolyzed using platinum electrodes. It can be concluded that the pH of the solution:
| 1. | Increases | 2. | Decreases |
| 3. | Unchanged | 4. | Can't be predicted |
Subtopic: Electrolytic & Electrochemical Cell |
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Kohlrausch gives the following relation for strong electrolytes:
\(\wedge=\wedge_{0}-A \sqrt{C}\)
Which of the following equality holds?
\(\text { 1. } \Lambda=\Lambda_{0} \text { as } C \longrightarrow \sqrt{\Lambda}\)
\(\text { 2. } \Lambda=\Lambda_{0} \text { as } C \longrightarrow \infty\)
\(\text { 3. } \Lambda=\Lambda_{0} \text { as } \mathrm{C} \longrightarrow 0\)
\(\text { 4. } \Lambda=\Lambda_{0} \text { as } C \longrightarrow 1\)
\(\wedge=\wedge_{0}-A \sqrt{C}\)
Which of the following equality holds?
\(\text { 1. } \Lambda=\Lambda_{0} \text { as } C \longrightarrow \sqrt{\Lambda}\)
\(\text { 2. } \Lambda=\Lambda_{0} \text { as } C \longrightarrow \infty\)
\(\text { 3. } \Lambda=\Lambda_{0} \text { as } \mathrm{C} \longrightarrow 0\)
\(\text { 4. } \Lambda=\Lambda_{0} \text { as } C \longrightarrow 1\)
Subtopic: Conductance & Conductivity | Kohlrausch Law & Cell Constant |
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The number of Faradays required for the deposition of 127 gram copper in copper sulphate solution is:
(Atomic weight of copper = 63.5)
1. 1 F
2. 2 F
3. 3 F
4. 4 F
(Atomic weight of copper = 63.5)
1. 1 F
2. 2 F
3. 3 F
4. 4 F
Subtopic: Faraday’s Law of Electrolysis |
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The correct statement regarding dry cells among the following is:
| a. | It is also known as the Leclanche cell. |
| b. | The electrolyte is a moist paste of ammonium chloride (NH4Cl) and zinc chloride (ZnCl2 ). |
| c. | The cathodic reaction is : MnO2 + NH4++ e-→ MnO(OH) + NH3 |
| 1. | Only a and b are correct | 2. | Only c is correct |
| 3. | Only b and c are correct | 4. | All are correct |
Subtopic: Batteries & Salt Bridge |
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Resistance of a decimolar solution between two electrodes 0.02 meter apart and 0.004 m2 in the area was found to be 50 ohms. Specific conductance (\(\)k) is :
1. \(0.1 Sm^{-1}\)
2. \(1 Sm^{-1}\)
3. \(10~ S~m^{-1}\)
4. \(4 \times 10^{-4} S~m^{-1}\)
1. \(0.1 Sm^{-1}\)
2. \(1 Sm^{-1}\)
3. \(10~ S~m^{-1}\)
4. \(4 \times 10^{-4} S~m^{-1}\)
Subtopic: Conductance & Conductivity |
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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 |
56%
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The potential of hydrogen electrode in contact with a solution with pH =10, is:
1. −0.0591 V2. −5.91 V
2. 0.0591 V
4. −0.591 V
Subtopic: Relation between Emf, G, Kc & pH |
73%
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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%
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NEET - 2022
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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 |
80%
From NCERT
NEET - 2022
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