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 |
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
If hydrogen electrodes dipped in two solutions of pH = 4 and pH = 6 are connected by a salt bridge, the emf of the resulting cell is -
1. 0.177 V
2. 0.3 V
3. 0.118 V
4. 0.104 V
Calculate the Emf of the given cell:
Zn(s) | Zn+2 (0.1M) || Sn+2 (0.001M) | Sn(s)
(Given
1. 0.62 V
2. 0.56 V
3. 1.12 V
4. 0.31 V
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 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.
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
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 |
1. | 17.6 mg | 2. | 21.3 mg |
3. | 24.3 mg | 4. | 13.6 mg |
The efficiency of a fuel cell is given by:
1.
2.
3.
4.