Proven Strategies to Ace Thermodynamics Mock Tests for JEE Main
Thermodynamics is a high-weightage chapter in JEE Physics, testing your grasp over critical laws of energy, heat transfer, work, and entropy. Mastering these core concepts will not only strengthen your fundamentals but also unlock your problem-solving edge for engineering entrance exams. Take this targeted mock test to boost confidence and reinforce your thermodynamics concepts!
Mock Test Instructions for the Thermodynamics Mock Test-3:
- 20 questions from Thermodynamics
- Time limit: 20 minutes
- Single correct answer per question
- Correct answers appear in bold green after submission
How Can JEE Mock Tests Help You Master Thermodynamics?
- Identify and correct misconceptions in thermodynamics laws and energy transfer through practice mock tests.
- Track progress with time-bound mocks and focus preparation on key exam patterns.
- Refine your approach to solving problems on entropy, heat transfer, and thermodynamic cycles with targeted MCQs.
- Enhance speed and accuracy in thermodynamics numericals by simulating real JEE scenarios.
- Use instant feedback from mock tests to target revision and improve weak areas in your understanding.
Master the Laws of Thermodynamics with Expert-Designed JEE Mock Tests
- Test your knowledge of the First and Second Laws of Thermodynamics with JEE-level questions.
- Understand concepts like heat, work, and internal energy using fully-explained answers in the mock test.
- Increase confidence in solving Carnot engine and entropy-based questions under exam pressure.
- Consolidate retention of essential formulas and units by repeated practice on thermodynamics problems.
- Get chapter-focused feedback to adapt your study plan for maximum marks in Physics.
Subject-Wise Excellence: JEE Main Mock Test Links
| S.No. | Subject-Specific JEE Main Online Mock Tests |
|---|---|
| 1 | Online FREE Mock Test for JEE Main Chemistry |
| 2 | Online FREE Mock Test for JEE Main Maths |
| 3 | Online FREE Mock Test for JEE Main Physics |
Important Study Materials Links for JEE Exams
FAQs on Thermodynamics Mock Test for JEE Main 2025-26: Practice & Preparation Guide
1. What is the first law of thermodynamics?
The first law of thermodynamics states that energy can neither be created nor destroyed, but can be converted from one form to another. It is also known as the law of conservation of energy. Mathematically, it is expressed as ΔU = Q − W, where ΔU is the change in internal energy, Q is the heat supplied to the system, and W is the work done by the system.
2. What is an isothermal process?
An isothermal process is a thermodynamic process in which the temperature of the system remains constant throughout. During this process, any heat supplied to the system is used to do work, and the internal energy remains unchanged.
3. How does the second law of thermodynamics differ from the first law?
The first law of thermodynamics deals with the conservation of energy, while the second law introduces the concept of entropy and the natural direction of processes. The second law states that the total entropy of an isolated system always increases over time, meaning energy conversions are not 100% efficient.
4. What is entropy in thermodynamics?
In thermodynamics, entropy is a measure of the degree of disorder or randomness in a system. It indicates the direction of spontaneous processes, with higher entropy meaning higher disorder. During irreversible processes, the entropy of a system increases.
5. What is meant by a thermodynamic system and its types?
A thermodynamic system is a defined quantity of matter or region in space which is under study, separated from its surroundings by real or imaginary boundaries. Types of systems include:
• Open System: Exchange both matter and energy with surroundings (e.g., boiling water in an open vessel).
• Closed System: Exchange energy but not matter (e.g., steam in a closed piston).
• Isolated System: No exchange of matter or energy (e.g., a thermos flask).
6. What is the difference between heat and work in thermodynamics?
In thermodynamics, heat is the energy transfer due to temperature difference between a system and its surroundings, while work is the energy transfer resulting from force acting over a distance. Both are ways energy can cross the boundary of a system, but their origins and effects differ.
7. Explain the concept of internal energy.
Internal energy is the total energy contained within a system, arising from the kinetic and potential energies of the molecules. It changes when heat is added or removed, or when work is done by or on the system.
8. What are state functions and path functions? Give examples.
State functions are properties that depend only on the current state of the system, not on the path taken (e.g., pressure, temperature, volume, internal energy). Path functions depend on the process followed to arrive at a state, such as heat (Q) and work (W).
9. What is a cyclic process?
A cyclic process is a thermodynamic process in which the system returns to its initial state after completing a sequence of changes. In a cyclic process, the net change in internal energy is zero, and the total work done equals the total heat supplied.
10. Explain the concept of reversible and irreversible processes.
A reversible process is one that can be reversed by an infinitesimal change, always remaining in thermodynamic equilibrium. Irreversible processes involve spontaneous changes and cannot be exactly reversed, often accompanied by an increase in entropy.
11. How is the efficiency of a Carnot engine defined?
The efficiency of a Carnot engine is the ratio of work done by the engine to the heat absorbed from the hot reservoir. Mathematically, efficiency (η) is:
• η = (Th – Tc)/Th
where Th is the temperature of the hot reservoir, and Tc is the temperature of the cold reservoir. Carnot engine has the maximum possible efficiency for any heat engine.
12. What is the significance of the zeroth law of thermodynamics?
The zeroth law of thermodynamics states that if two systems are each in thermal equilibrium with a third system, then they are also in thermal equilibrium with each other. This law forms the basis of the concept of temperature and allows us to use thermometers for temperature measurement.
