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Q. No.Which reaction is NOT a redox reaction?
1. \(2 \mathrm{KClO}_3+\mathrm{I}_2 \rightarrow 2 \mathrm{KIO}_3+\mathrm{Cl}_2\)
2. \(\mathrm{H}_2+\mathrm{Cl}_2 \rightarrow 2 \mathrm{HCl}\)
3. \(\mathrm{BaCl}_2+\mathrm{Na}_2 \mathrm{SO}_4 \rightarrow \mathrm{BaSO}_4+2 \mathrm{NaCl}\)
4. \(\mathrm{Zn}+\mathrm{CuSO}_4 \rightarrow \mathrm{ZnSO}_4+\mathrm{Cu}\)
1. \(2 \mathrm{KClO}_3+\mathrm{I}_2 \rightarrow 2 \mathrm{KIO}_3+\mathrm{Cl}_2\)
2. \(\mathrm{H}_2+\mathrm{Cl}_2 \rightarrow 2 \mathrm{HCl}\)
3. \(\mathrm{BaCl}_2+\mathrm{Na}_2 \mathrm{SO}_4 \rightarrow \mathrm{BaSO}_4+2 \mathrm{NaCl}\)
4. \(\mathrm{Zn}+\mathrm{CuSO}_4 \rightarrow \mathrm{ZnSO}_4+\mathrm{Cu}\)
Subtopic: Introduction to Redox and Oxidation Number |
65%
Level 2: 60%+
NEET - 2024
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At \(298 {~K},\) the standard electrode potentials of \(\mathrm{{Cu}^{2+} /{Cu},}\) \(\mathrm{{Zn}^{2+} / {Zn},~~ {Fe}^{2+} / {Fe}}\) and \(\mathrm{{Ag}^{+} / {Ag}} \) are \(\mathrm{0.34 {~V}, -0.76 {~V},}\) \(\mathrm{-0.44 {~V}}\) and \(\mathrm{0.80 {~V},}\) respectively.
On the basis of standard electrode potentials, predict which of the following reaction can not occur?
On the basis of standard electrode potentials, predict which of the following reaction can not occur?
| 1. | \(\mathrm{2 {CuSO}_{4}({aq})+2 {Ag}({s}) → 2 {Cu}({s})+{Ag}_{2} {SO}_{4}({aq})} \) |
| 2. | \(\mathrm{{CuSO}_{4}({aq})+{Zn}({s})} \) \(\mathrm{→ {ZnSO}_{4}({aq})+{Cu}({s})} \) |
| 3. | \(\mathrm{{CuSO}_{4}({aq})+{Fe}({s})} \) \(\mathrm{→ {FeSO}_{4}({aq})+{Cu}({s})} \) |
| 4. | \(\mathrm{{FeSO}_{4}({aq})+{Zn}({s})} \) \(→ \mathrm{{ZnSO}_{4}({aq})+{Fe}({s})} \) |
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
The oxidation states of the central atom in the given species are, respectively:
| 1. | 0 and +6 | 2. | +3 and +4 |
| 3. | +4 and +2 | 4. | +5 and +6 |
Subtopic: Introduction to Redox and Oxidation Number |
91%
Level 1: 80%+
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KI3, H2S4O6
The oxidation numbers of iodine and sulphur in the above compounds are, respectively:
| 1. | \(\dfrac{1}{3}\); 4 | 2. | 2.5 ; \(\dfrac{1}{3}\) |
| 3. | \(-\dfrac{1}{3}\); 2.5 | 4. | 2.5 ; 3 |
Subtopic: Introduction to Redox and Oxidation Number |
89%
Level 1: 80%+
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Subtopic: Introduction to Redox and Oxidation Number |
85%
Level 1: 80%+
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Why does the MnO₄²⁻ ion undergo disproportionation in an acidic medium, whereas the MnO₄⁻ ion does not?
| 1. | Due to manganese being in its highest oxidation state in MnO₄²⁻. |
| 2. | Due to manganese being in its highest oxidation state in MnO₄⁻ |
| 3. | Because the disproportionation reaction of MnO₄²⁻ is endothermic. |
| 4. | Because the disproportionation reaction of MnO₄²⁻ is exothermic. |
Subtopic: Introduction to Redox and Oxidation Number |
81%
Level 1: 80%+
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Subtopic: Introduction to Redox and Oxidation Number |
75%
Level 2: 60%+
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Given below are two statements:
| Assertion (A): | In the representation Fe³⁺/Fe²⁺, Ce⁴⁺/Ce³⁺ , and Cu²⁺/Cu, each pair represents a redox couple. |
| Reason (R): | A redox couple is the combination of the oxidised and reduced forms of a substance involved in an oxidation or reduction half-cell. |
| 1. | Both (A) and (R) are True and (R) is the correct explanation of (A). |
| 2. | Both (A) and (R) are True, but (R) is not the correct explanation of (A). |
| 3. | (A) is True but (R) is False. |
| 4. | (A) is False but (R) is True. |
Subtopic: Introduction to Redox and Oxidation Number |
74%
Level 2: 60%+
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The oxidation number of sulphur and nitrogen in H2SO5 and NO3- are respectively-
| 1. | +6, +5 | 2. | -6, -6 |
| 3. | +8, +6 | 4. | -8, -6 |
Subtopic: Introduction to Redox and Oxidation Number |
77%
Level 2: 60%+
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