The oxidation states of the central atom in the given species are, respectively:

H4P2O7  and H2S2O7

1. 0 and +6 2. +3 and +4
3. +4 and +2 4. +5 and +6

Subtopic:  Introduction to Redox and Oxidation Number |
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KI3, H2S4O6

The oxidation numbers of iodine and sulphur in the above compounds are, respectively:

1. \(\frac{1}{3}\) ; 4
2. 2.5 ; \(\frac{1}{3}\)
3. \(-\frac{1}{3}\) ; 2.5
4. 2.5 ; 3

Subtopic:  Introduction to Redox and Oxidation Number |
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The oxidising agent and reducing agent in the given reaction are :

Cl2O7g+4H2O2aq+2OHaq-
2ClO2aq-+4O2g+5H2Ol

1. Oxidizing agent = H2O2; Reducing agent = Cl2O7

2. Oxidizing agent = Cl2O7; Reducing agent = H2O2

3. Oxidizing agent = H2O2; Reducing agent = H2O2

4. None of the above

Subtopic:  Oxidizing & Reducing Agents |
 80%
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The oxidizing agent and reducing agent in the given reaction are :

3N2H4l+4ClO3aq-
6NOg+4Claq-+6H2Ol

1. Oxidising agent = N2H4; Reducing agent = ClO3-

2. Oxidising agent = ClO3-; Reducing agent = N2H4

3. Oxidising agent = N2H4 ; Reducing agent = N2H4

4. Oxidising agent = ClO3- ; Reducing agent = ClO3-

Subtopic:  Oxidizing & Reducing Agents |
 83%
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The correct statement about electrolysis of an aqueous solution of CuCl2 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 

Subtopic:  Emf & Electrode Potential |
 66%
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The correct statement about the electrolysis of an aqueous solution of AgNO3 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

Subtopic:  Emf & Electrode Potential |
 61%
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Consider the given data:

EFe3+/Fe2+=0.77; EI-/I2= -0.54
EAg+/Ag=0.80; ECu/Cu2+= -0.34
EFe3+/Fe2+=0.77; ECu/Cu2+= -0.34
EAg/Ag+=-0.80; EFe3+/Fe2+=0.77

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)

Subtopic:  Application of Electrode Potential |
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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
Subtopic:  Balancing of Equations |
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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)

Subtopic:  Balancing of Equations |
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The oxidising agent and reducing agent in the given reaction are

5P4s+12H2Ol+12HO-aq
8PH3g+12HPO2-aq

1. Oxidising agent = P4; Reducing agent = P4

2. Oxidising agent = P4; Reducing agent = H2O

3. Oxidising agent = H2O; Reducing agent = P4

4. None of the above

Subtopic:  Redox Titration & Type of Redox |
 69%
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