Pairs of reactants (R) and product (P) are given below. The pair which can be used in a fuel cell is :
1.
2.
3.
4.
The cell that will measure the standard electrode potential of a copper electrode is:
1. | \(1 \over 10\) bar) | H+(aq, 1M) || Cu2+(aq, 1M) | Cu Pt(s) | H2(g, |
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. | \(1 \over 10\) bar) | H+(aq, \(1 \over 10\)M) || Cu2+(aq, 1M) | Cu Pt(s) | H2(g, |
For the electrolysis of CuSO4 solution the correct option is:
1. Cathode reaction: Cu2+ + 2e- Cu using Cu electrode.
2. Anode reaction: Cu Cu+ + e- using Cu electrode.
3. Cathode reaction: 2H+ + 2e- H2 using Pt electrode.
4. Anode reaction: Cu Cu2+ + 2e- using Pt electrode.
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- ; \(E_{cell}^{o}\)
During discharge of a lead storage cell, the density of sulphuric acid in the cell-
1. Increases.
2. Decreases.
3. Remains unchanged.
4. Initially increases but decreases subsequently.
On electrolysis of dilute sulphuric acid using Platinum (Pt) electrode, the product obtained at the anode will be:
1. Oxygen gas
2. gas
3. gas
4. Hydrogen gas
An electrochemical cell can behave like an electrolytic cell when -
1. Ecell = 0
2. Ecell > Eext
3. Eext > Ecell
4. Ecell = Eext
The correct statement about the given galvanic cell equation is -
Zn(s) + 2Ag+(aq) → Zn2+(aq) + 2Ag(s)
1. | The current will flow from silver to zinc in the external circuit. |
2. | The current will flow from zinc to silver in the external circuit. |
3. | The current will flow from silver to zinc in the internal circuit. |
4. | The current will flow from zinc to silver in the internal circuit. |
When aqueous NaCl solution is electrolysed using inert electrodes then pH of the solution-
1. Increases.
2. Decreases.
3. Remains same.
4. First increases then decreases.
Salt with the highest electrolytic conductivity in solution is :
1. K2[PtCl6]
2. [Co(NH3)3(NO2)3]
3. K4[Fe(CN)6]
4. [Co(NH3)4]SO4