11th Chemistry Thermodynamics MCQ Quiz for 2026 exam

Challenge yourself with our 11th grade Chemistry Thermodynamics MCQ quiz. Master key concepts of heat, energy, and thermal processes in chemical systems.

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Time: 10 Minutes for 10 Question.

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11th Chemistry: Thermodynamics

1 / 10

1. Which of the following defines a thermodynamic system?

A part of the universe where observations are made

Everything other than the part of the universe under observation

The combination of system and surroundings

The part of the universe that includes the surroundings only

2 / 10

2. What does a large equilibrium constant (K) indicate for a reaction?

The reaction is endothermic

The reaction is exothermic

The reaction does not go to completion

The reaction has a high activation energy

3 / 10

3. What does Hess’s Law state about the enthalpy change of a reaction?

It depends on the path of the reaction

It is independent of the path of the reaction

It varies with pressure changes

It varies with volume changes

4 / 10

4. What is the heat absorbed or evolved at constant pressure also called?

Internal energy

Gibbs energy

Work function

Enthalpy of reaction

5 / 10

5. Which is a macroscopic property used in thermodynamics?

Atomic radius

Molecular mass

Pressure

Bond length

6 / 10

6. Which law of thermodynamics applies to the energy changes of a system moving from one equilibrium state to another?

Zeroth Law

First Law

Second Law

Third Law

7 / 10

7. Which process is spontaneous at all temperatures?

One with positive ?H and negative ?S

One with negative ?H and positive ?S

One with positive ?H and positive ?S

One with negative ?H and negative ?S

8 / 10

8. What is the enthalpy change for the combustion of graphite to form CO2?

+110.5 kJ/mol

-110.5 kJ/mol

-393.5 kJ/mol

+393.5 kJ/mol

9 / 10

9. Which term refers to the energy changes of macroscopic systems?

Kinetics

Thermodynamics

Equilibrium

Dynamics

10 / 10

10. What does the standard enthalpy of reaction depend on?

Pressure only

Temperature only

Conditions under which the reaction is carried out

Volume only

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View Chapter wise MCQ Quiz of 11th Chemistry

Chapter of 11th Chemistry Chapter Wise MCQ

Unit 1 Some Basic Concepts of Chemistry
1.1 Importance of Chemistry
1.2 Nature of Matter
1.3 Properties of Matter and their Measurement
1.4 Uncertainty in Measurement
1.5 Laws of Chemical Combinations
1.6 Dalton’s Atomic Theory
1.7 Atomic and Molecular Masses
1.8 Mole Concept and Molar Masses
1.9 Percentage Composition
1.10 Stoichiometry and Stoichiometric Calculations

Unit 2 Structure of Atom
2.1 Discovery of Sub-atomic Particles
2.2 Atomic Models
2.3 Developments Leading to the Bohr’s Model of Atom
2.4 Bohr’s Model for Hydrogen Atom
2.5 Towards Quantum Mechanical Model of the Atom
2.6 Quantum Mechanical Model of Atom

Unit 3 Classification of Elements and Periodicity in Properties
3.1 Why do we Need to Classify Elements ?
3.2 Genesis of Periodic Classification
3.3 Modern Periodic Law and the Present Form of the Periodic Table
3.4 Nomenclature of Elements with Atomic Numbers > 100
3.5 Electronic Configurations of Elements and the Periodic Table
3.6 Electronic Configurations and Types of Elements: s-, p-, d-, f- Blocks
3.7 Periodic Trends in Properties of Elements

Unit 4 Chemical Bonding and Molecular Structure
4.1 Kössel-Lewis Approach to Chemical Bonding
4.2 Ionic or Electrovalent Bond
4.3 Bond Parameters
4.4 The Valence Shell Electron Pair Repulsion (VSEPR) Theory
4.5 Valence Bond Theory
4.6 Hybridisation
4.7 Molecular Orbital Theory
4.8 Bonding in Some Homonuclear Diatomic Molecules
4.9 Hydrogen Bonding

Unit 5 Thermodynamics
5.1 Thermodynamic Terms
5.2 Applications
5.3 Measurement of ÄU and ÄH: Calorimetry
5.4 Enthalpy Change, ÄrH of a Reaction – Reaction Enthalpy
5.5 Enthalpies for Different Types of Reactions
5.6 Spontaneity
5.7 Gibbs Energy Change and Equilibrium

Unit 6 Equilibrium
6.1 Equilibrium in Physical Processes
6.2 Equilibrium in Chemical Processes – Dynamic Equilibrium
6.3 Law of Chemical Equilibrium and Equilibrium Constant
6.4 Homogeneous Equilibria
6.5 Heterogeneous Equilibria
6.6 Applications of Equilibrium Constants
6.7 Relationship between Equilibrium Constant K, Reaction Quotient Q and Gibbs Energy G
6.8 Factors Affecting Equilibria
6.9 Ionic Equilibrium in Solution
6.10 Acids, Bases and Salts
6.11 Ionization of Acids and Bases
6.12 Buffer Solutions
6.13 Solubility Equilibria of Sparingly Soluble Salts

Study Source:

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