Q. No.An electrochemical cell can behave like an electrolytic cell when -
1. Ecell = 0
2. Ecell > Eext
3. Eext > Ecell
4. Ecell = Eext
The incorrect statement about the solution of electrolytes is:
| 1. | Conductivity of solution depends upon the size of ions. |
| 2. | Conductivity depends upon the viscosity of solution. |
| 3. | Conductivity does not depend upon the solvation of ions present in solution. |
| 4. | Conductivity of solution increases with temperature. |
The most stable oxidized species among the following is:
\(E_{{\mathrm{Cr}_2 \mathrm{O}_7^2}/ \mathrm{Cr}^{3+}}^{o} =1.33 \mathrm{~V} ; E_{\mathrm{Cl}_2 / \mathrm{Cl}^{-}}^{o}=1.36 \mathrm{~V} \)
\( E_{\mathrm{MnO_{4}}^{-} / \mathrm{Mn}^{2+}}^{o}=1.51 \mathrm{~V} ; E_{\mathrm{Cr}^{3+} / \mathrm{Cr}}^{o}=-0.74 \mathrm{~V}\)
| 1. | Cr3+ | 2. | MnO4- |
| 3. | Cr2O72- | 4. | Mn2+ |
The quantity of charge required to obtain one mole of aluminium from Al2O3 is :
1. 1 F
2. 6 F
3. 3 F
4. 2 F
The cell constant of a conductivity cell-
| 1. | Changes with the change of electrolyte. |
| 2. | Changes with the change of concentration of electrolyte. |
| 3. | Changes with the temperature of the electrolyte. |
| 4. | Remains constant for a cell. |
| 1. | PbSO4 anode is reduced to Pb. |
| 2. | PbSO4 cathode is reduced to Pb. |
| 3. | PbSO4 cathode is oxidised to Pb. |
| 4. | PbSO4 anode is oxidised to PbO2. |
\(\Lambda _{m(NH_{4}OH)}^{o}\) is equal to -
1. \(\Lambda _{m(NH_{4}OH)}^{o} \ + \ \Lambda _{m(NH_{4}Cl)}^{o} \ - \ \Lambda _{m(HCl)}^{o}\)
2. \(\Lambda _{m(NH_{4}Cl)}^{o} \ + \ \Lambda _{m(NaOH)}^{o} \ - \ \Lambda _{m(NaCl)}^{o}\)
3. \(\Lambda _{m(NH_{4}Cl)}^{o} \ + \ \Lambda _{m(NaCl)}^{o} \ - \ \Lambda _{m(NaOH)}^{o}\)
4. \(\ \Lambda _{m(NaOH)}^{o} \ + \ \Lambda _{m(NaCl)}^{o}\ - \ \Lambda _{m(NH_{4}Cl)}^{o}\)
The half-cell reaction at the anode during the electrolysis of aqueous sodium chloride solution is represented by :
1. Na+(aq) + e- ⟶ Na(s) ; \(E_{cell}^{o} \ = \ -2.71 \ V \)
2. 2H2O(l) ⟶ O2(g) + 4H+(aq) + 4e- ; \(E_{cell}^{o} \) = 1.23 V
3. H+(aq) + e- ⟶ \(\frac{1}{2}\)H2(g) ; \(E_{cell}^{o} \) = 0.00 V
4. Cl-(aq) ⟶ \(\frac{1}{2}\)Cl2(g) + e- ; \(E_{cell}^{o}\)
Match the terms given in Column I with the items given in Column II.
|
Column I |
Column II |
|
A. B. Eocell C. D. Gcell |
1. Intensive property 2. Depends on number of ions/volume 3. Extensive property 4. Increases with dilution |
Codes:
| Options: | A | B | C | D |
| 1. | 2 | 3 | 4 | 1 |
| 2. | 1 | 2 | 3 | 5 |
| 3. | 5 | 4 | 3 | 2 |
| 4. | 4 | 1 | 2 | 3 |
Given below are two statements:
| Assertion (A): | Current stops flowing when Ecell = 0. |
| Reason (R): | Equilibrium of the cell reaction is attained. |
| 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. |
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