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 statements in the balanced equation are:
a. Na is oxidized
b. H2 is oxidized
c. H2 is reduced
d. It is a disproportionation reaction
Choose the correct option:
| 1. | a and b | 2. | b and c |
| 3. | a and c | 4. | a and d |
For the reaction:
Fe3O4 (s) + Al (s) → Fe (s) + Al2O3 (s)
Which of the following statements about the reaction are correct?
| a. | Stoichiometric coefficient of Fe is 9. |
| b. | Aluminium is oxidized. |
| c. | Ferrous ferric oxide (Fe3O4) is oxidized. |
| 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 |
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 | 4. | c = 1; d = 1; f = 1 |
In the following equation, the products A and B are, respectively are:
\(\small Cr_2O^{2-}_7 (aq) + 3SO^{2-}_3 (aq) + 8H^+(aq) \rightarrow A + B + 4H_2O(l)\)
1. \(2 \mathrm{Cr}^{2+} ; 3 \mathrm{SO}_2 \)
2. \(2 \mathrm{Cr}^{+} ; \mathrm{S}_2 \mathrm{O}_7{ }^{2-} \)
3. \(2 \mathrm{Cr}^{3+} ; 3 \mathrm{SO}_4{ }^{2-} \)
4. \(2 \mathrm{Cr}^{3+} ; 3 \mathrm{HSO}_4{ }^{-}\)
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 |
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. \(ClO_{3}^{-}\)
© 2026 GoodEd Technologies Pvt. Ltd.