Kohlrausch's law states that at:
1. | Finite dilution, each ion makes definite contribution to equivalent conductance of an electrolyte, whatever be the nature of the other ion of the electrolyte. |
2. | Infinite dilution, each ion makes definite contribution to equivalent conductance of an electrolyte depending on the nature of the other ion of the electrolyte. |
3. | Infinite dilution, each ion makes definite contribution to conductance of an electrolyte whatever be the nature of the other ion of the electrolyte. |
4. | Infinite dilution, each ion makes definite contribution to equivalent conductance of an electrolyte, whatever be the nature of the other ion of the electrolyte. |
A steady current of 1.5 A flows through a copper voltmeter for 10 min. If the electrochemical equivalent of copper is 30 × 10-5 g C-1, the mass of copper deposited on the electrode will be:
1. 0.40 g
2. 0.50 g
3. 0.67 g
4. 0.27 g
The efficiency of a fuel cell is given by:
1.
2.
3.
4.
1. | 17.6 mg | 2. | 21.3 mg |
3. | 24.3 mg | 4. | 13.6 mg |
If = -0.441 V and = 0.771 V, the standard emf of the reaction:
Fe + 2Fe3+→ 3Fe2+ will be:
1. | 0.330 V | 2. | 1.653 V |
3. | 1.212 V | 4. | 0.111 V |
A hypothetical electrochemical cell is shown below.
A|A+(x M) || B+(y M)|B
The Emf measured is +0.20 V. The cell reaction is:
1. A+ + B → A + B+
2. A+ + e- → A ; B+ + e- → B
3. The cell reaction cannot be predicted.
4. A + B+ → A+ + B
For the cell reaction
\(\mathrm{2Fe^{3+}(aq) \ + \ 2I^{-}(aq)\rightarrow 2Fe^{2+}(aq) \ + \ I_{2}(aq)}\)
\(E_{cell}^{o} \ = \ 0.24 \ V\) at . The standard Gibbs energy ∆rG⊝ of the cell reaction is:
[Given: ]
1.
2.
3.
4.
For a cell involving one electron at 298 K.
The equilibrium constant for the cell reaction is :
\(\mathrm{[Given~ that~ \frac {2.303 ~RT}{F} = 0.059 ~V~ at~ T = 298 K]}\)
1.
2.
3.
4.
For a reaction A(s) + 2B+ A2+ + 2B(s) ; KC has been found to be 1012. The is :
1. | 0.35 V | 2. | 0.71 V |
3. | 0.01 V | 4. | 1.36 V |