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Q. No.Which of the following cannot as an oxidising agent?
1. \(\mathrm{MnO}_4^{-}\)
2. \(\mathrm{SO}_4^{2-}\)
3. \(\mathrm{N}^{3-}\)
4. \(\mathrm{BrO}_3^{-}\)
Subtopic: Oxidizing & Reducing Agents |
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Level 2: 60%+
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Balance the following chemical equation and choose the option with the correct set of values of x, y, z, and p:
\(\mathrm{xCl}_2+\mathrm{yOH}^{-} \longrightarrow \mathrm{zCl}^{-}+\mathrm{pClO}^{-}\)
1. \(\text{x}=1,\text{y}=2,\text{z}=2,\text{p}=1\)
2. \(\text{x}=\text{y}=\text{z}=\text{p}=1\)
3. \(\text{x}=1,\text{y}=1,\text{z}=2,\text{p}=1\)
4. \(\text{x}=1,\text{y}=2,\text{z}=1,\text{p}=1\)
\(\mathrm{xCl}_2+\mathrm{yOH}^{-} \longrightarrow \mathrm{zCl}^{-}+\mathrm{pClO}^{-}\)
1. \(\text{x}=1,\text{y}=2,\text{z}=2,\text{p}=1\)
2. \(\text{x}=\text{y}=\text{z}=\text{p}=1\)
3. \(\text{x}=1,\text{y}=1,\text{z}=2,\text{p}=1\)
4. \(\text{x}=1,\text{y}=2,\text{z}=1,\text{p}=1\)
Subtopic: Balancing of Equations |
Level 3: 35%-60%
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Among the following, how many metal ions act as oxidising agents?
\(\mathrm{Sn}^{2+}, \mathrm{Sn}^{4+}, \mathrm{Pb}^{4+}, \mathrm{Pb}^{2+}, \mathrm{Tl}^{+}, \mathrm{Tl}^{3+}\)
1. 2
2. 4
3. 1
4. 0
\(\mathrm{Sn}^{2+}, \mathrm{Sn}^{4+}, \mathrm{Pb}^{4+}, \mathrm{Pb}^{2+}, \mathrm{Tl}^{+}, \mathrm{Tl}^{3+}\)
1. 2
2. 4
3. 1
4. 0
Subtopic: Oxidizing & Reducing Agents |
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The species given below that does not show a disproportionation reaction is:
| 1. | \(\text{BrO}^-\) | 2. | \(\text{BrO}^-_4\) |
| 3. | \(\text{BrO}^-_3\) | 4. | \(\text{BrO}^-_2\) |
Subtopic: Introduction to Redox and Oxidation Number |
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Match the redox reactions in List-I with their corresponding type of redox reaction in List-II.
Choose the correct answer from the options given below :
1. A-II, B-III, C-IV, D-I
2. A-II, B-III, C-I, D-IV
3. A-III, B-IV, C-I, D-II
4. A-IV, B-I, C-II, D-III
| List-I (Redox Reaction) |
List-II (Type of Redox Reaction) |
||
| (A) | \(\mathrm{CH}_{4(\mathrm{~g})}+2 \mathrm{O}_{2(\mathrm{~g})}\) \(\xrightarrow{\Delta} \mathrm{CO}_{2(\mathrm{~g})}+\) \(2 \mathrm{H}_2 \mathrm{O}_{(1)}\) | (I) | Disproportionation reaction |
| (B) | \(2 \mathrm{NaH}_{(\mathrm{s})} \xrightarrow{\Delta}\) \(2 \mathrm{Na}_{(\mathrm{s})}+\mathrm{H}_{2(\mathrm{~g})}\) | (II) | Combination reaction |
| (C) | \(\mathrm{V}_2 \mathrm{O}_{5(\mathrm{~s})}+5 \mathrm{Ca}_{(\mathrm{s})}\) \(\xrightarrow{\Delta} 2 \mathrm{~V}_{(\mathrm{s})} ~+\) \(5 \mathrm{CaO}_{(\mathrm{s}}\) | (III) | Decomposition reaction |
| (D) | \(2 \mathrm{H}_2 \mathrm{O}_{2(\mathrm{aq})} \xrightarrow{\Delta}\) \(2 \mathrm{H}_2 \mathrm{O}_{(1)}+\mathrm{O}_{2(\mathrm{~g})}\) | (IV) | Displacement reaction |
Choose the correct answer from the options given below :
1. A-II, B-III, C-IV, D-I
2. A-II, B-III, C-I, D-IV
3. A-III, B-IV, C-I, D-II
4. A-IV, B-I, C-II, D-III
Subtopic: Introduction to Redox and Oxidation Number |
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Consider the given standard electrode potentials:
\(\mathrm{E}_{\mathrm{Cr}_2 \mathrm{O}_7^{2-} / \mathrm{Cr}^{3+}}^0=1.33 \mathrm{~V}\) \(\mathrm{E}_{\mathrm{Cl}_2 / \mathrm{Cl}^{(-)}}^0=1.36 \mathrm{~V}\)
\(\mathrm{E}_{\mathrm{MnO}_4^{-} / \mathrm{Mn}^{2+}}^0=1.51 \mathrm{~V}\) \(\mathrm{E}_{\mathrm{Cr}^{3+} / \mathrm{Cr}}^0=-0.74 \mathrm{~V}\)
The strongest reducing agent is:
\(\mathrm{E}_{\mathrm{Cr}_2 \mathrm{O}_7^{2-} / \mathrm{Cr}^{3+}}^0=1.33 \mathrm{~V}\) \(\mathrm{E}_{\mathrm{Cl}_2 / \mathrm{Cl}^{(-)}}^0=1.36 \mathrm{~V}\)
\(\mathrm{E}_{\mathrm{MnO}_4^{-} / \mathrm{Mn}^{2+}}^0=1.51 \mathrm{~V}\) \(\mathrm{E}_{\mathrm{Cr}^{3+} / \mathrm{Cr}}^0=-0.74 \mathrm{~V}\)
The strongest reducing agent is:
| 1. | \(\mathrm{Mn}^{2+}\) | 2. | Cr |
| 3. | \(\mathrm{MnO}_4^{-}\) | 4. | \(\mathrm{Cl}^{-}\) |
Subtopic: Oxidizing & Reducing Agents |
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Which of the following can show disproportionation reaction?
1. \(MnO^-_4\)
2. \(ClO^-_4\)
3. \(MnO^{2-}_4\)
4. \(F_2\)
1. \(MnO^-_4\)
2. \(ClO^-_4\)
3. \(MnO^{2-}_4\)
4. \(F_2\)
Subtopic: Redox Titration & Type of Redox |
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Which one of the following is an example of a disproportionation reaction?
| 1. | \(\small{3 \mathrm{MnO}_{4}^{2-}+4 \mathrm{H}^{+} \rightarrow 2 \mathrm{MnO}_{4}^{-}+\mathrm{MnO}_{2}+2 \mathrm{H}_{2} \mathrm{O}}\) |
| 2. | \(\small{\mathrm{MnO}_{4}^{-}+4 \mathrm{H}^{+}+4 e^{-} \rightarrow \mathrm{MnO}_{2}+2 \mathrm{H}_{2} \mathrm{O}}\) |
| 3. | \(\small{10 \mathrm{I}^{-}+2 \mathrm{MnO}_{4}^{-}+16 \mathrm{H}^{+} \rightarrow 2 \mathrm{Mn}^{2+}+8 \mathrm{H}_{2} \mathrm{O}+5 \mathrm{I}_{2}}\) |
| 4. | \(\small{8 \mathrm{MnO}_{4}^{-}+3 \mathrm{~S}_{2} \mathrm{O}_{3}^{2-}+\mathrm{H}_{2} \mathrm{O} \rightarrow 8 \mathrm{MnO}_{2}+6 \mathrm{SO}_{4}^{2-}+2 \mathrm{OH}^{-}}\) |
Subtopic: Redox Titration & Type of Redox |
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Standard reduction electrode potentials of three metals A, B and C are +0.5V , -3.0 V and -1.2 V respectively. The reducing power of these metals are:
| 1. | B >C > A | 2. | A >B > C |
| 3. | C > B >A | 4. | A > C > B |
Subtopic: Emf & Electrode Potential |
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What is the oxidation number of Cl in \(\text{CaOCl}_2\) (bleaching powder)?
1. Zero, because it contains Cl2
2. -1, because it contains Cl-
3. +1, because it contains ClO-
4. +1 and -1 because it contains ClO- and Cl-
Subtopic: Introduction to Redox and Oxidation Number |
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