Standard reduction potentials of the half-reactions are given below:
The strongest oxidizing and reducing agents, respectively, are:
1. and
2. and
3. and
4. and
Fluorine reacts with ice as per the following reaction
H2O(s) + F2(g) → HF(g) + HOF(g)
This reaction is a redox reaction because-
1. | F2 is getting oxidized. | 2. | F2 is getting reduced. |
3. | Both (1) and (2)
|
4. | None of the above. |
The formulas for the following compounds are:
(a) Mercury(II) chloride and (b) Thallium(I) sulphate
1. HgCl2, Tl2SO4
2. Hg2Cl2, Tl2SO4
3. HgCl2, TlSO4
4. HgCl2, Tl3SO4
The correct statement(s) about the given reaction is -
\(\mathrm{{X} eO_{6 (aq)}^{4 -} + 2 F^{- 1}_{(aq)} + 6 H^{+}_{(aq )} \rightarrow}~\mathrm{{X} eO_{3 (g)} + {F}_{2 (g)} + 3 H_{2} O_{(l)}}\)
1. oxidises F-
2. The oxidation number of F increases from -1 to zero
3. is a stronger oxidizing agent that
4. All of the above.
The oxidising agent and reducing agent in the given reaction are
1. Oxidising agent = ; Reducing agent =
2. Oxidising agent = ; Reducing agent =
3. Oxidising agent = ; Reducing agent =
4. None of the above
The balanced equation for the reaction between chlorine and sulphur dioxide in water is:
1. | Cl2(s) + SO2(aq) + 2H2O(I) →2Cl-(aq) + SO42-(aq) + 4H+(aq) |
2. | 3Cl2(s) + SO2(aq) + 2H2O(I) →Cl-(aq) + SO42-(aq) + 3H+(aq) |
3. | Cl2(s) + 3SO2(aq) + H2O(I) →Cl-(aq) + 2SO42-(aq) + 4H+(aq) |
4. | 2Cl2(s) + SO2(aq) + H2O(I) →2Cl-(aq) + SO42-(aq) + 4H+(aq) |
The maximum weight of nitric oxide that can be obtained starting only with 10.00 g of ammonia and 20.00 g of oxygen is:
1. | 9 g | 2. | 15 g |
3. | 12 g | 4. | 11g |
Consider the given data:
Using the electrode potential values given above, identify the reaction which is not feasible:
1. | Fe3+(aq) and I- aq) |
2. | Ag+(aq) and Cu(s) |
3. | Fe3+(aq) and Cu(s) |
4. | Ag(s) and Fe3+(aq) |
The correct statement about the electrolysis of an aqueous solution of with Pt electrode is:
1. | Pt(s) gets oxidized at cathode whereas Ag + ( aq ) gets reduced at anode |
2. | Ag+ (aq) gets reduced at cathode and is oxidized at anode |
3. | Ag+ (aq) gets reduced at cathode whereas water is oxidized at anode |
4. | Ag (s) gets oxidized at cathode whereas H2O is oxidised at anode |
The correct statement about electrolysis of an aqueous solution of with Pt electrode is-
1. | Cu2+ ion reduced at the cathode; Cl- ion oxidized at the anode |
2. | Cu2+ ion reduced at the anode; Cl- ion oxidized at the cathode |
3. | Cu2+ ion reduced at the cathode; H2O ion oxidized at the anode |
4. | H2O ion reduced at the cathode; Cl- ion oxidized at the anode |