Chapter 7: Redox Reactions MCQs | chemistry Class 11 CBSE

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Chapter 7: Redox Reactions MCQs | chemistry Class 11 CBSE | ByteNotes.in

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Question 1

Objective

In the reaction 2Mg(s) + O2(g) → 2MgO(s), magnesium is said to be oxidised because:

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Question 2

Objective

Which of the following best defines a reducing agent in terms of electron transfer?

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Question 3

Objective

The oxidation number of chromium in K2Cr2O7 is:

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Question 4

Objective

The oxidation number of oxygen in KO2 (potassium superoxide) is:

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Question 5

Objective

In the reaction Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s), the oxidising agent is:

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Question 6

Objective

Which of the following reactions is an example of a disproportionation reaction?

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Question 7

Objective

In the Half-Reaction method, for a reaction occurring in basic medium, after balancing atoms and charge using H+ and H2O, the next step is to:

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Question 8

Objective

The standard electrode potential of the hydrogen electrode is taken as:

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Question 9

Objective

In the Daniell cell, which electrode is the negative electrode (anode)?

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Question 10

Objective

Which of the following halogens is the strongest oxidising agent?

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Question 11

Objective

The oxidation number of sulphur in H2SO4 is:

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Question 12

Objective

In the reaction 2KClO3 → 2KCl + 3O2, the change in oxidation number of chlorine is:

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Question 13

Objective

A metal activity series shows the electron-releasing tendency in the order Zn > Cu > Ag. When copper metal is placed in silver nitrate solution, the observation is:

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Question 14

Objective

Which of the following oxoanions of chlorine CANNOT undergo disproportionation?

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Question 15

Objective

In the reaction CH4 + 4Cl2 → CCl4 + 4HCl, the oxidation number of carbon changes from:

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Question 16

Objective

The salt bridge in the Daniell cell contains KCl or NH4NO3. Its primary function is to:

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Question 17

Objective

In which of the following compounds does hydrogen have an oxidation number of -1?

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Question 18

Objective

The reaction Cl2(g) + 2OH-(aq) → ClO-(aq) + Cl-(aq) + H2O(l) is used industrially to produce:

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Question 19

Objective

In a redox titration, permanganate ion (MnO4-) is described as a self-indicator because:

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Question 20

Objective

The standard electrode potential of Zn2+/Zn is -0.76 V. This means that:

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Chapter 7: Redox Reactions | MCQs

In the reaction 2Mg(s) + O2(g) → 2MgO(s), magnesium is said to be oxidised because:

Which of the following best defines a reducing agent in terms of electron transfer?

The oxidation number of chromium in K2Cr2O7 is:

The oxidation number of oxygen in KO2 (potassium superoxide) is:

In the reaction Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s), the oxidising agent is:

Which of the following reactions is an example of a disproportionation reaction?

In the Half-Reaction method, for a reaction occurring in basic medium, after balancing atoms and charge using H+ and H2O, the next step is to:

The standard electrode potential of the hydrogen electrode is taken as:

In the Daniell cell, which electrode is the negative electrode (anode)?

Which of the following halogens is the strongest oxidising agent?

The oxidation number of sulphur in H2SO4 is:

In the reaction 2KClO3 → 2KCl + 3O2, the change in oxidation number of chlorine is:

A metal activity series shows the electron-releasing tendency in the order Zn > Cu > Ag. When copper metal is placed in silver nitrate solution, the observation is:

Which of the following oxoanions of chlorine CANNOT undergo disproportionation?

In the reaction CH4 + 4Cl2 → CCl4 + 4HCl, the oxidation number of carbon changes from:

The salt bridge in the Daniell cell contains KCl or NH4NO3. Its primary function is to:

In which of the following compounds does hydrogen have an oxidation number of -1?

The reaction Cl2(g) + 2OH-(aq) → ClO-(aq) + Cl-(aq) + H2O(l) is used industrially to produce:

In a redox titration, permanganate ion (MnO4-) is described as a self-indicator because:

The standard electrode potential of Zn2+/Zn is -0.76 V. This means that:

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