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 |
The oxidizing 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. Oxidising agent = ; Reducing agent =
The oxidising agent and reducing agent in the given reaction are :
1. Oxidizing agent = H2O2; Reducing agent =
2. Oxidizing agent = ; Reducing agent =
3. Oxidizing agent = H2O2; Reducing agent = H2O2
4. None of the above
The oxidation states of the central atom in the given species are, respectively:
1. | 0 and +6 | 2. | +3 and +4 |
3. | +4 and +2 | 4. | +5 and +6 |
KI3, H2S4O6
The oxidation numbers of iodine and sulphur in the above compounds are, respectively:
1. \(\dfrac{1}{3}\) ; 4
2. 2.5 ; \(\dfrac{1}{3}\)
3. \(-\dfrac{1}{3}\) ; 2.5
4. 2.5 ; 3
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