CBSE Class 11 Chemistry Part 2 by Pavan | Practice Test to Test Your Knowledge
Students

Academic Programs

AI-powered learning for grades 8-12, aligned with major curricula

Engineering Courses
Professional

Professional Courses

Industry-relevant training in Business, Technology, and Design

Certifications
Games

Interactive Games

Fun games to boost memory, math, typing, and English skills

  2. Practice Tests
  3. CBSE Class 11 Chemistry Part 2
CBSE Class 11 Chemistry Part 2

CBSE Class 11 Chemistry Part 2

Thorough mock test on Acids and Bases, Metals and Non-metals, and Organic Chemistry. Includes chemical reactions, laboratory techniques, and industrial applications.

2025-07-17
Pavan Pavan
CBSE Class 11 Grade 11 Chemistry

Duration

30 min

Questions

30

Marking

Negative

You've not yet enrolled in this practice test. Please login to start practice test.

Questions Preview

What is the main characteristic of a redox reaction?

A
Involves both oxidation and reduction occurring simultaneously
B
Involves the addition of oxygen to a substance
C
Involves the removal of hydrogen from a substance
D
Involves only the oxidation of a substance

Which of the following is an example of an oxidation reaction?

A
2 Mg (s) + O2 (g) → 2 MgO (s)
B
2 FeCl3 (aq) + H2 (g) → 2 FeCl2 (aq) + 2 HCl (aq)
C
2 H2O (l) → 2 H2 (g) + O2 (g)
D
CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (l)

What happens during a reduction reaction?

A
An atom or ion gains electrons
B
An atom or ion loses electrons
C
Oxygen is added to the substance
D
Hydrogen is removed from the substance

Which of the following compounds has an oxidation number of +1 for sulfur?

A
H2SO4
B
Na2SO4
C
SO2
D
H2S

What is the role of sodium in the reaction 2 Na (s) + H2 (g) → 2 NaH (s)?

A
Sodium is oxidized
B
Sodium is reduced
C
Sodium is neither oxidized nor reduced
D
Sodium acts as an oxidizing agent

In a redox reaction, which of the following species acts as an oxidizing agent?

A
The species that gains electrons
B
The species that loses electrons
C
The species that donates electrons
D
The species that is reduced

Which of the following reactions is an example of a displacement redox reaction?

A
CuSO4(aq) + Zn(s) → Cu(s) + ZnSO4(aq)
B
H2 + O2 → H2O
C
NaH + H2O → NaOH + H2
D
C(s) + O2(g) → CO2(g)

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

A
2H2O2(aq) → 2H2O(l) + O2(g)
B
2Na(s) + Cl2(g) → 2NaCl(s)
C
Mg(s) + 2H2O(l) → Mg(OH)2(aq) + H2(g)
D
C(s) + 2O2(g) → CO2(g)

In the reaction, 2Na + Cl2 → 2NaCl, what happens to sodium (Na)?

A
Sodium is oxidized
B
Sodium is reduced
C
Sodium acts as an oxidizing agent
D
Sodium remains unaffected

Which of the following reactions is an example of a combination redox reaction?

A
C(s) + O2(g) → CO2(g)
B
2H2O(l) → 2H2(g) + O2(g)
C
CaCO3(s) → CaO(s) + CO2(g)
D
2Na(s) + H2O(l) → 2NaOH(aq) + H2(g)

Which element undergoes reduction in the reaction: 2Na(s) + Cl2(g) → 2NaCl(s)?

A
Sodium (Na)
B
Chlorine (Cl)
C
Neither sodium nor chlorine
D
Both sodium and chlorine

Which of the following is an example of a redox reaction that involves hydrogen?

A
H2 + O2 → H2O
B
2Na(s) + H2O(l) → 2NaOH(aq) + H2(g)
C
CH4 + 2O2 → CO2 + 2H2O
D
2H2S + O2 → 2H2O + 2S

What is the oxidation number of chlorine in NaCl?

A
-1
B
0
C
+1
D
+2

Which of the following is true about the oxidation number of oxygen?

A
In most compounds, oxygen has an oxidation number of -2
B
Oxygen always has an oxidation number of -1
C
Oxygen always has an oxidation number of +1
D
Oxygen has a variable oxidation number depending on the compound

In the reaction 2FeCl3 + 3Zn → 2Fe + 3ZnCl2, which element is reduced?

A
Iron (Fe)
B
Zinc (Zn)
C
Chlorine (Cl)
D
None

Which of the following is not a type of redox reaction?

A
Combination reaction
B
Decomposition reaction
C
Displacement reaction
D
Neutralization reaction

What is the oxidation number of sulfur in SO2?

A
+4
B
-2
C
0
D
+6

Which of the following elements has the highest oxidation state in its compounds?

A
Sulfur
B
Oxygen
C
Chlorine
D
Fluorine

What is the role of the salt bridge in a redox reaction?

A
To allow ions to flow between two solutions, completing the circuit
B
To provide a source of electrons
C
To balance the oxidation reactions
D
To generate electricity

Which of the following reactions can be used in a galvanic cell?

A
Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)
B
Na(s) + Cl2(g) → NaCl(s)
C
2Na + H2 → 2NaH
D
C(s) + O2(g) → CO2(g)

Which of the following metals has the lowest tendency to release electrons?

A
Copper
B
Zinc
C
Iron
D
Magnesium

Which of the following is true about redox reactions?

A
Oxidation occurs by the loss of electrons
B
Reduction occurs by the loss of electrons
C
Oxidizing agents lose electrons
D
Redox reactions only occur in acidic solutions

In a Galvanic cell, what happens at the anode?

A
Oxidation occurs
B
Reduction occurs
C
The flow of electrons stops
D
The salt bridge is dissolved

Which of the following reactions is an example of a redox reaction in a basic medium?

A
MnO4–(aq) + 2H2O(l) → MnO2(s) + 4OH–(aq)
B
H2SO4(aq) + NaOH(aq) → Na2SO4(aq) + H2O(l)
C
2Na(s) + Cl2(g) → 2NaCl(s)
D
CH4(g) + O2(g) → CO2(g) + 2H2O(l)

What is the purpose of using an indicator in redox titration?

A
To show the end point of the reaction
B
To accelerate the reaction
C
To increase the concentration of reactants
D
To decrease the concentration of products

In the redox reaction between zinc and copper sulfate (Zn + CuSO4 → Cu + ZnSO4), what happens to zinc?

A
Zinc is oxidized
B
Zinc is reduced
C
Zinc acts as the oxidizing agent
D
Zinc remains unchanged

Which of the following is a product of the redox reaction between hydrogen peroxide and sodium iodide?

A
Iodine
B
Sodium chloride
C
Water
D
Sodium iodide

What happens to chlorine in the reaction Cl2 + 2e– → 2Cl–?

A
Chlorine is reduced
B
Chlorine is oxidized
C
Chlorine remains unchanged
D
Chlorine is neutralized

Which metal is more reactive based on its ability to lose electrons in a redox reaction?

A
Magnesium
B
Iron
C
Copper
D
Silver

What type of reaction is demonstrated by the equation: 2H2O2 → 2H2O + O2?

A
Decomposition redox reaction
B
Combination redox reaction
C
Displacement redox reaction
D
Disproportionation redox reaction