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Q. No.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:
1.
\(\mathrm{Mn}^{2+}\)
2.
Cr
3.
\(\mathrm{MnO}_4^{-}\)
4.
\(\mathrm{Cl}^{-}\)
Subtopic: Oxidizing & Reducing Agents |
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Level 2: 60%+
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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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Level 1: 80%+
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Find the value of x when 15 mL of an acidic aqueous Fe²⁺ solution completely reacts with 20 mL of 0.03 M K₂Cr₂O₇ solution.
The molarity of the Fe²⁺ solution is expressed as x × 10⁻² M.
(Round off x to the nearest integer.)
1. 14
2. 20
3. 24
4. 30
The molarity of the Fe²⁺ solution is expressed as x × 10⁻² M.
(Round off x to the nearest integer.)
1. 14
2. 20
3. 24
4. 30
Subtopic: Redox Titration & Type of Redox |
85%
Level 1: 80%+
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\(10.0 ~\text{mL}\) of \(\mathrm{Na_2CO_3}\) solution is titrated against \(0.2~\text{M HCl}\) solution. The following titre value of 5 readings were recorded :
\(\text{4.8 ml, 4.9 ml, 5.0 ml, 5.1 ml and 5.0 ml}\)
Based on these readings, and convention of titrimetric estimation the concentration of \(\mathrm{Na_2CO_3}\) solution in mM is: (Round off to the Nearest Integer).
1. 25
2. 50
3. 60
4. 85
\(\text{4.8 ml, 4.9 ml, 5.0 ml, 5.1 ml and 5.0 ml}\)
Based on these readings, and convention of titrimetric estimation the concentration of \(\mathrm{Na_2CO_3}\) solution in mM is: (Round off to the Nearest Integer).
1. 25
2. 50
3. 60
4. 85
Subtopic: Redox Titration & Type of Redox |
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Level 2: 60%+
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Identify the process in which a change in the oxidation state is five:
1. \(\mathrm{MnO}_4^{-} \rightarrow \mathrm{Mn}^{2+}\)
2. \(\mathrm{CrO}_4^{2-} \rightarrow \mathrm{Cr}^{3+}\)
3. \(\mathrm{C}_2 \mathrm{O}_4^{2-} \rightarrow 2 \mathrm{CO}_2\)
4. \(\mathrm{Cr}_2 \mathrm{O}_7^{2-} \rightarrow 2 \mathrm{Cr}^{3+}\)
1. \(\mathrm{MnO}_4^{-} \rightarrow \mathrm{Mn}^{2+}\)
2. \(\mathrm{CrO}_4^{2-} \rightarrow \mathrm{Cr}^{3+}\)
3. \(\mathrm{C}_2 \mathrm{O}_4^{2-} \rightarrow 2 \mathrm{CO}_2\)
4. \(\mathrm{Cr}_2 \mathrm{O}_7^{2-} \rightarrow 2 \mathrm{Cr}^{3+}\)
Subtopic: Oxidizing & Reducing Agents |
91%
Level 1: 80%+
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Which one of the following forms when \(\text{Cu}^{2+}\) salt reacts with potassium iodide?
1. \(\text{CuI}\)
2. \(\mathrm{Cu_2I_2}\)
3. \(\mathrm{Cu(I_3)_2}\)
4. \(\mathrm{Cu_2I_3}\)
Subtopic: Redox Titration & Type of Redox |
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Among the following, which is the strongest oxidizing agent?
1. \(Mn^{3+}\)
2. \(Fe^{3+}\)
3. \(Ti^{3+}\)
4. \(Cr^{3+}\)
1. \(Mn^{3+}\)
2. \(Fe^{3+}\)
3. \(Ti^{3+}\)
4. \(Cr^{3+}\)
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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Find the sol produced when AgNO₃ solution is added to the KI solution from the following options:
1. AgI/Ag⁺
2. KI/NO₃⁻
3. AgNO₃/NO₃⁻
4. AgI/I⁻
Subtopic: Redox Titration & Type of Redox |
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Level 3: 35%-60%
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Which of the following sets of species contains only those that can undergo a disproportionation reaction?
| 1. | \(\mathrm{ClO_2^-,MnO^-_4}\) and \(\mathrm{CrO^{2-}_{7}}\) |
| 2. | \(\mathrm{ClO_2^-}\) and \(\mathrm{Mn^{3+}}\) |
| 3. | \(\mathrm{ClO^-_4,MnO^-_4}\)and \(\mathrm{ClO^-_2}\) |
| 4. | \(\mathrm{Cr_2O^{2-}_7,MnO^-_4}\) and \(\mathrm{Cl_2}\) |
Subtopic: Redox Titration & Type of Redox |
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Level 2: 60%+
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