The pressure of H2 required to make the potential of H2 - electrode zero in pure water at 298 K is:
1. | 10–12 atm | 2. | 10–10 atm |
3. | 10–4 atm | 4. | 10–14 atm |
When 0.1 mol MnO42– is oxidized, the quantity of electricity required to completely oxidise MnO42– to MnO4– is:
1. 96500 C
2. 2 × 96500 C
3. 9650 C
4. 96.50 C
Zn2+(aq) + 2e–→ Zn(s) | Eo = – 0.76 V |
Ag2O(s) + H2O(l) + 2e– → 2Ag(s) + 2OH–(aq) | Eo = 0.34 V |
The cell potential will be:
1. | 0.42 V | 2. | 0.84 V |
3. | 1.34 V | 4. | 1.10 V |
Cu2+(aq) + e- → Cu+(aq) | 0.15 V |
Cu+(aq) + e- → Cu(s) | 0.50 V |
1. | 0.325 V | 2. | 0650 V |
3. | 0.150 V | 4. | 0.500 V |
The molar conductance of solution of a weak monobasic acid is 8.0 ohm-1 cm2 and at infinite dilution is 400 ohm-1 cm2. The dissociation constant of this acid is:
1. | \(1.25 \times10^{-5}\) | 2. | \(1.25 \times10^{-6}\) |
3. | \(6.25 \times10^{-4}\) | 4. | \(1.25 \times10^{-4}\) |
Given:
(i) Eo = 0.337 V
(ii) Eo = 0.153 V
Electrode potential, Eo for the reaction,
, will be:
1. 0.52 V
2. 0.90 V
3. 0.30 V
4. 0.38 V
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 |
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.
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4.