Q. No.The standard electrode potential for Sn4+/Sn2+ couple is +0.15 V and that for the Cr3+/Cr couple is -0.74 V. These two couples in their standard state are connected to make a cell. The cell potential will be:
| 1. | +0.89 V | 2. | +0.18 V |
| 3. | +1.83 V | 4. | +1.199 V |
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Zn(s) + Ag2O(s) + H2O(l) \(\rightleftharpoons\) 2Ag(s) + Zn2+(aq) + 2OH–(aq)
If half-cell potentials are-
| 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 |
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Molten sodium chloride conducts electricity due to the presence of:
1. Free ions.
2. Free molecules.
3. Free electrons.
4. Atoms of sodium and chlorine.
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The metal that cannot be produced upon reduction of its oxide by aluminium is :
| 1. | K | 2. | Mn |
| 3. | Cr | 4. | Fe |
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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 |
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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. |
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Consider the change in the oxidation state of Bromine corresponding to different emf values as shown in the diagram below:
\(\small{BrO_4^-\ \overset{1.82V}{\longrightarrow}\ BrO_3^-\ \overset{1.5V}{\longrightarrow} HBrO\ \overset{1.595V}{\longrightarrow}\ Br_2 \overset{1.0652V}{\longrightarrow}\ Br^-}\)
Then the species undergoing disproportionation is:-
1.
2.
3.
4. HBrO
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| Cu2+(aq) + e- → Cu+(aq) | 0.15 V |
| Cu+(aq) + e- → Cu(s) | 0.50 V |
The value of \(E_{Cu^{2+}/Cu}^{o}\) will be:
| 1. | 0.325 V | 2. | 0650 V |
| 3. | 0.150 V | 4. | 0.500 V |
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The standard reduction potential for Fe2+|Fe and Sn2+|Sn electrodes are -0.44 V and -0.14 V respectively. For the cell reaction,
Fe2+ + Sn → Fe + Sn2+, the standard Emf is -
1. +0.30 V
2. 0.58 V
3. +0.58 V
4. -0.30 V
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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
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