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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MnO42- undergoes disproportionation reaction in acidic medium but MnO4- does not. It is:

1.  Due to the highest oxidation state of Mn in  MnO42-
2.  Due to the highest oxidation state of Mn in  MnO4-
3.  Due to the endothermic nature of the disproportionation reaction.
4.  Due to the exothermic nature of the disproportionation reaction.

Subtopic:  Introduction to Redox and Oxidation Number |
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The reaction that does not represent auto redox or disproportionation is: 

1. Cl2+OH-Cl-+ClO3-+H2O

2. 2H2O2H2O+O2

3. 2Cu+Cu2++Cu

4. NH42Cr2O7N2+Cr2O3+4H2O

Subtopic:  Introduction to Redox and Oxidation Number |
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Which of the following reactions does not represent a redox change?

1. CaCO3 CaO + CO2

2. 2H2 + O2 2H2O

3. Na + H2 NaOH + \(\frac{1}{2}\)H2

4. MnCl3  MnCl2 + \(\frac{1}{2}\)Cl2

Subtopic:  Introduction to Redox and Oxidation Number |
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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.
 

Subtopic:  Introduction to Redox and Oxidation Number |
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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

Subtopic:  Introduction to Redox and Oxidation Number |
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In the given balanced chemical reaction,


\(\mathrm{IO}_3^{-}+\mathrm{aI}^{-}+\mathrm{bH}^{+} \rightarrow \mathrm{cH}_2 \mathrm{O}+\mathrm{dI}_2\)

The values of a, b, c, and d respectively are-

1. 5, 6, 3, 3

2. 5, 3, 6, 3

3. 3, 5, 3, 6

4. 5, 6, 5, 5

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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For the redox reaction,
 aMnO4-+bC2O42-+cH+dMn2++eCO2+fH2O
the correct stoichiometric coefficients of the reactants a, b, and c respectively for the balanced equation are: 

1. 16, 5, 2
2. 2, 5, 16
3. 2, 16, 5
4. 5, 16, 2

Subtopic:  Balancing of Equations |
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