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 |
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 |
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 |
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 |
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. \(ClO_{3}^{-}\)