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Q. No.x & y are the number of moles of electrons involved respectively during oxidation of \(I^-\) to \(I_2\) & \(S^{2-}\) to S by acidified \({K}_2 {Cr}_2 {O}_7 .\) The value of x+y is?
1. 10
2. 12
3. 16
4. 18
1. 10
2. 12
3. 16
4. 18
Subtopic: Balancing of Equations |
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Hints
If \(\mathrm{K}_2 \mathrm{Cr}_2 \mathrm{O}_7\left(200 \mathrm{~cm}^3, \mathrm{x} \times 10^{-3} \mathrm{M}\right)\) reacts with Mohr's salt \( (0.6 \text M~,750~\text{cm}^3)\) then find the value of x:
1. 125
2. 250
3. 375
4. 750
1. 125
2. 250
3. 375
4. 750
Subtopic: Oxidizing & Reducing Agents | Redox Titration & Type of Redox |
73%
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 |
80%
Level 1: 80%+
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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 |
71%
Level 2: 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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Level 2: 60%+
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In which of the following compound \(Mn\) will have highest oxidation state?
1. \(\mathrm{MnO}_4^{-}\)
2. \(\mathrm{MnO}_2\)
3. \(\mathrm{MnO}_4^{2-}\)
4. \(\mathrm{Mn}_2 \mathrm{O}_3\)
1. \(\mathrm{MnO}_4^{-}\)
2. \(\mathrm{MnO}_2\)
3. \(\mathrm{MnO}_4^{2-}\)
4. \(\mathrm{Mn}_2 \mathrm{O}_3\)
Subtopic: Introduction to Redox and Oxidation Number |
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Level 1: 80%+
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50 mL of KMnO4 solution is used for titration with 20 mL of 2M oxalic acid solution in Acidic medium. The molarity of KMnO4 solution is x × 10–2 M. The value of x is:
1. 32
2. 35
3. 26
4. 94
1. 32
2. 35
3. 26
4. 94
Subtopic: Redox Titration & Type of Redox |
80%
Level 1: 80%+
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Which of the following undergoes disproportionation reaction in aqueous alkaline medium?
| 1. | \(\mathrm{I}_2~ \text {and}~ \mathrm{Cl}_2\) only | 2. | \(\mathrm{F}_2~\text {and}~\mathrm{Cl}_2\) only |
| 3. | \(\mathrm{I}_2~\text {and}~\mathrm{Br}_2\) only | 4. | \(\mathrm{Cl}_2, \mathrm{Br}_2~\text {and}~\mathrm{I}_2\) only |
Subtopic: Redox Titration & Type of Redox |
68%
Level 2: 60%+
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The number of moles of \(\text{H}^+\) required by 1 mole \( \text{MnO}^-_4\) to oxidize oxalate ion to \( \text{CO}_2\) is are:
1. 8
2. 4
3. 10
4. 7
1. 8
2. 4
3. 10
4. 7
Subtopic: Balancing of Equations |
54%
Level 3: 35%-60%
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\(\mathrm{Cr}_2 \mathrm{O}_7^{2-}+\mathrm{xH}^{+}+\mathrm{ye}^{-} \rightarrow 2 \mathrm{Cr}^{3+}+\mathrm{AH}_2 \mathrm{O}\)
Balance the above reaction and find \(\text{x,y}~ \text{and} ~\text{A}\):
1. \(\text{x}=7,\text{y}=6,\text{A}=14\)
2. \(\text{x}=14,\text{y}=6,\text{A}=7\)
3. \(\text{x}=14,\text{y}=3,\text{A}=7\)
4. \(\text{x}=8,\text{y}=2,\text{A}=1\)
Balance the above reaction and find \(\text{x,y}~ \text{and} ~\text{A}\):
1. \(\text{x}=7,\text{y}=6,\text{A}=14\)
2. \(\text{x}=14,\text{y}=6,\text{A}=7\)
3. \(\text{x}=14,\text{y}=3,\text{A}=7\)
4. \(\text{x}=8,\text{y}=2,\text{A}=1\)
Subtopic: Balancing of Equations |
81%
Level 1: 80%+
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