Q. No.Mg(s) | Mg2+(0.001M) || Cu2+(0.0001 M) | Cu(s)
The value of for the above reaction is -
1.
3.46 V
2.
3.15 V
3.
2.67 V
4.
1.24 V
The cell that will measure the standard electrode potential of a copper electrode is:
| 1. | Pt(s) | H2(g, \(1 \over 10\) bar) | H+(aq, 1M) || Cu2+(aq, 1M) | Cu |
| 2. | Pt(s) | H2(g, 1 bar) | H+(aq, 1M) || Cu2+ (aq, 2M) | Cu |
| 3. | Pt(s) | H2(g, 1 bar) | H+(aq, 1M)|| Cu2+ (aq, 1M) | Cu |
| 4. | Pt(s) | H2(g, \(1 \over 10\) bar) | H+(aq, \(1 \over 10\)M) || Cu2+(aq, 1M) | Cu |
The electrode potential for Mg electrode varies according to the equation
\(E_{Mg^{2+}/Mg}\ = \ E_{Mg^{2+}/Mg}^{o} \ - \ \frac{0.059}{2}log\frac{1}{[Mg^{2+}]}\)
The graph of EMg2+ / Mg vs log [Mg2+] among the following is:
| 1. |  |
2. |  |
| 3. |  |
4. |  |
The correct statement among the following options is:
| 1. | Ecell and ∆rG of cell reaction are both extensive properties. |
| 2. | Ecell and ∆rG of cell reaction are both intensive properties. |
| 3. | Ecell is an intensive property while ∆rG of cell reaction is an extensive property. |
| 4. | Ecell is an extensive property while ∆rG of cell reaction is an intensive property. |
The difference between the electrode potentials of two electrodes when no current is drawn through the cell is called:
1. Cell potential.
2. Cell emf.
3. Potential difference.
4. Cell voltage.
The incorrect statement about an inert electrode in a cell is:
| 1. | It does not participate in the cell reaction. |
| 2. | It provides a surface either for oxidation or for the reduction reaction. |
| 3. | It provides a surface for the conduction of electrons. |
| 4. | It provides a surface for redox reaction. |
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
© 2025 GoodEd Technologies Pvt. Ltd.