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Q. No.The given-below reaction can be classified as:
\(2PbO + 4HNO_3 \rightarrow 2Pb(NO_3)_2 + 2H_2O\)
1. Combination reaction
2. Redox reaction
3. Acid-base reaction
4. Disproportion reaction
Subtopic: Redox Titration & Type of Redox |
57%
Level 3: 35%-60%
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Subtopic: Introduction to Redox and Oxidation Number |
80%
Level 1: 80%+
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Identify the oxidant (O) and reductant (R) in the following reaction:
\(Pb_3O_4 + 8HCl \rightarrow 3PbCl_2 + Cl_2 + 4H_2O \)
1. \(\mathrm{{O}={PbO}}, \ \mathrm{{R}= {Cl}^{-}} \)
2. \(\mathrm{{O}={PbO}_2}, \ \mathrm{{R}= {PbO}} \)
3. \(\mathrm{{O}={PbO}}, \ \mathrm{{R}= {PbO}_2} \)
4. \(\mathrm{{O}={PbO}_2}, \ \mathrm{{R}= {Cl}^{-}}\)
\(Pb_3O_4 + 8HCl \rightarrow 3PbCl_2 + Cl_2 + 4H_2O \)
1. \(\mathrm{{O}={PbO}}, \ \mathrm{{R}= {Cl}^{-}} \)
2. \(\mathrm{{O}={PbO}_2}, \ \mathrm{{R}= {PbO}} \)
3. \(\mathrm{{O}={PbO}}, \ \mathrm{{R}= {PbO}_2} \)
4. \(\mathrm{{O}={PbO}_2}, \ \mathrm{{R}= {Cl}^{-}}\)
Subtopic: Oxidizing & Reducing Agents |
70%
Level 2: 60%+
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Which of the following reactions is a decomposition redox reaction?
| 1. | \(\mathrm{2 {Pb}\left({NO}_3\right)_2({s}) \rightarrow 2 {PbO}({s})+4 {NO}_2({g})+{O}_2({g})} \) |
| 2. | \(\mathrm{{N}_2({g})+{O}_2({g}) \rightarrow 2 {NO}({g})} \) |
| 3. | \(\small{\mathrm{{Cl}_2({g})+2 {OH}^{-}({aq}) \rightarrow {ClO}^{-}({aq})+{Cl}^{-}({aq})+4 {H}_2 {O}(\ell)}}\) |
| 4. | \(\small{\mathrm{{P}_4({s})+3 {OH}^{-}({aq})+3 {H}_2 {O}(\ell) \rightarrow{PH}_3({g})+3 {H}_2 {PO}_2^{-}({aq})}}\) |
Subtopic: Redox Titration & Type of Redox |
73%
Level 2: 60%+
NEET - 2022
Hints
A set of species capable of showing disproportionation reactions is:
| 1. | \(\mathrm{ClO^–_2, ~ClO^–_3,~ ClO^–_4, ~Cl_2}\) |
| 2. | \(\mathrm{Cl_2, ~ClO^–_2, ~ClO^–_3, ~S_8}\) |
| 3. | \(\mathrm{ClO^–_4, ~ClO^–, ~ClO^–_2, ~F_2}\) |
| 4. | \(\mathrm{ClO^–_3, ~ClO^–_4, ~H_2O_2, ~ClO^–}\) |
Subtopic: Redox Titration & Type of Redox |
62%
Level 2: 60%+
NEET - 2022
Hints
Which of the following redox reactions is thermodynamically non-spontaneous under standard conditions at 298 K?
Given the standard reduction potentials:
E°(Cu²⁺/Cu) = +0.34 V
E°(Zn²⁺/Zn) = −0.76 V
E°(Fe²⁺/Fe) = −0.44 V
E°(Ag⁺/Ag) = +0.80 V
1. CuSO₄(aq) + 2Ag(s) → Cu(s) + Ag₂SO₄(aq)
2. CuSO₄(aq) + Zn(s) → ZnSO₄(aq) + Cu(s)
3. CuSO₄(aq) + Fe(s) → FeSO₄(aq) + Cu(s)
4. FeSO₄(aq) + Zn(s) → ZnSO₄(aq) + Fe(s)
Subtopic: Emf & Electrode Potential |
69%
Level 2: 60%+
NEET - 2022
Hints
Identify the incorrect statement from the following:
| 1. | Lithium is the strongest reducing agent among the alkali metals. |
| 2. | Alkali metals react with water to form their hydroxides. |
| 3. | The oxidation number of K in KO2 is +4. |
| 4. | Ionisation enthalpy of alkali metals decreases from top to bottom in the group. |
Subtopic: Introduction to Redox and Oxidation Number |
68%
Level 2: 60%+
NEET - 2022
Hints
For the given redox reaction, find out the coefficients a, b and c of a balanced equation respectively:
\(\mathrm{{a} {Cr}_2 {O}_7^{2-}+{bSO}_3^{2-}({aq})+{c} {H}^{+}({aq})} →\)\(\mathrm{2 {a} {Cr}^{3+}({aq})+{bSO}_4^{2-}({aq})+\frac{{c}}{2} {H}_2 {O}(\ell)} \)
\(\mathrm{{a} {Cr}_2 {O}_7^{2-}+{bSO}_3^{2-}({aq})+{c} {H}^{+}({aq})} →\)\(\mathrm{2 {a} {Cr}^{3+}({aq})+{bSO}_4^{2-}({aq})+\frac{{c}}{2} {H}_2 {O}(\ell)} \)
| 1. | 8, 1 and 3 | 2. | 1, 3 and 8 |
| 3. | 3, 8 and 1 | 4. | 1, 8 and 3 |
Subtopic: Balancing of Equations |
78%
Level 2: 60%+
NEET - 2023
Hints
The molar conductance of a solution, given its conductivity (0.248 S m–1) and concentration (0.2 mol m–3) is:
| 1. | 0.124 S cm2 mol–1 | 2. | 1.24 S m2 mol–1 |
| 3. | 124 S cm2 mol–1 | 4. | 124 S m2 mol–1 |
Subtopic: Conductance & Conductivity |
Level 3: 35%-60%
NEET - 2023
Hints
Find the element that is being reduced in the following redox reaction:
3Cu(s) + 8HNO₃(aq) → 2NO(g) + 3Cu(NO₃)₂(aq) + 4H₂O(l)
| 1. | Cu | 2. | H |
| 3. | N | 4. | O |
Subtopic: Oxidizing & Reducing Agents |
85%
Level 1: 80%+
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