Q. No.Consider the following reaction:
Pb3O4 + 4HNO3 → A + B + 2H2O
A and B are respectively-
1. A=Pb(NO3)4; B=PbO2
2. A=Pb; B=O2
3. A= Pb(NO3)2; B=PbO2
4. A=PbO; B=NO2
(O.S = oxidation state)
| Column I | Column II |
| a. Fe O.S in Fe2O3 | i. +2 |
| b. Mn O.S in MnO2 | ii. +3 |
| c. Mn O.S in MnO | iii. +4 |
1. a=i; b=ii; c=iii
2. a=ii; b=iii; c=i
3. a=iii; b=ii; c=i
4. a=ii; b=i; c=iii
2Na(s) + H2(g) → 2NaH(s)
The correct statement(s) in the balanced equation is(are):
a. Na is oxidized
b. H2 is oxidized
c. H2 is reduced
d. It is a disproportionation reaction
1. a, b
2. b, c
3. c, a
4. a, d
For the reaction:
Fe3O4 (s) + Al (s) → Fe (s) + Al2O3 (s)
The correct statement(s) in the equation is(are):
| a. | Stoichiometric coefficient of Fe is 9. |
| b. | Aluminium is oxidized |
| c. | Ferrous ferric oxide (Fe3O4) is oxidize |
| d. | Aluminium is reduced. |
1. a, c
2. a, b
3. b, c
4. c, d
Permanganate(VII) ion, MnO4– in basic solution oxidizes iodide ion, I– to produce molecular iodine (I2) and manganese (IV) oxide (MnO2). The reaction is as follows:
aI–(aq) + bMnO4–(aq) + cH2O(l) → dI2(s) + eMnO2(s) + fOH–(aq)
The value of b, d and f are-
1. b=2; d=3; f=8
2. b=1; d=3; f=8
3. b=3; d=8; f=2
4. b=8; d=3; f=2
aMnO4–(aq) + bBr–(aq) + cH2O(l) → dMnO2(s) + eBrO3– (aq) + fOH–(aq)
The value of c, d and f in the above mentioned reaction are respectively-
1. c=1; d=2; f=2
2. c=2; d=1; f=2
3. c=2; d=2; f=1
d. c=1; d=1; f=1
Consider the following equation:
Cr2O72–(aq) + 3SO32– (aq)+ 8H+(aq) → A + B +4H2O(l)
The product A and B are respectively-
1. 2Cr2+; 3SO2
2. 2Cr+; S2O7 2-
3. 2Cr3+; 3SO4 2-
4. 2Cr3+; 3HSO42-
Consider the following reaction:
Pb3O4 + 8HCl → A + B + 4H2O
A and B are, respectively,:
1. A= PbCl4; B= PbCl2
2. A= PbCl2; B= Cl2
3. A= PbCl4; B=Cl2
4. A = PbCl2; B = O2
Match the items in column I with the items in column II.
| Column I | Column II |
| a. N2 (g) + O2 (g) → 2 NO (g) | i. Disproportionation redox reaction |
| b. 2Pb(NO3)2(s) → 2PbO(s) + 4 NO2 (g) + O2 (g) | ii. Decomposition redox reaction |
| c. NaH(s) + H2O(l) → NaOH(aq) + H2 (g) | iii. Combination redox reactions |
| d. 2NO2(g) + 2OH–(aq) → NO2–(aq) + NO3– (aq) + H2O(l) | iv. Displacement redox reaction |
1. a=iii; b=ii; c=iv; d=i
2. a=iii; b=iv; c=i; d=ii
3. a=ii; b=iii; c=iv; d=i
4. a=iv; b=i; c=iii; d=ii
The species among the following that does not show a disproportionation reaction is-
ClO–, ClO2–, \(ClO_{3}^{-}\) and ClO4–
1. ClO–
2. ClO2–
3. ClO4–
4. \(ClO_{3}^{-}\)
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