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Kinetic Theory Of Gases for NEET: Practice and Mastery
The kinetic theory of gases is a vital topic in NEET Physics, offering deep insight into the molecular nature of matter and the origin of macroscopic properties like pressure and temperature. Aspirants aiming for top NEET 2026 ranks should focus on concept-based MCQs, time management, and error reduction within this chapter.
Why Attempt Kinetic Theory Of Gases Mock Tests?
Practicing NEET mock tests on the Kinetic Theory Of Gases allows students to get familiar with actual exam patterns, identify weak concepts, and build confidence. Mock tests with instant scoring, solutions, and analytics simulate the real NEET experience, boosting exam readiness efficiently.
Key Concepts in Kinetic Theory Of Gases
The major concepts tested include postulates of kinetic theory, pressure-molecular collisions, equipartition of energy, and specific heats. Understanding mean free path, velocity distribution, ideal and real gases, and the mathematical relations is essential for securing marks in NEET Physics chapters.
| Formula/Concept | Description |
|---|---|
| Average Kinetic Energy per Molecule | <KE> = (3/2)kT, where k = Boltzmann constant, T = absolute temperature |
| Ideal Gas Equation | PV = nRT; relates pressure, volume, moles, and temperature |
| Root Mean Square Speed | urms = √(3RT/M), where M = molar mass |
| van der Waals Equation | (P + a(n/V)2)(V - nb) = nRT; for real gases |
Benefits of Chapter-Wise Practice for NEET 2026
Focusing on chapter-specific mock tests like this Kinetic Theory Of Gases Mock Test 3 helps you pinpoint learning gaps. You receive instant feedback, track scoring trends, and refine strategies for full-length NEET mock exams, resulting in steady improvement with each attempt.
Key Features: NEET Kinetic Theory Of Gases Online Mock Test 3
- Strictly NTA-patterned 20 MCQs for fast, focused practice
- Timer-based test (20 minutes) to sharpen exam speed and accuracy
- Detailed solutions and instant scoring for all questions
- Analytics: See correct, incorrect, and unanswered questions
- Device-friendly – available on mobile and desktop
- Unlimited reattempts for concept mastery
Exam Performance Tracking and Self-Analysis
After submission, your score, accuracy, and solution breakdown empower you to identify strengths and weaknesses. Chapter-wise analytics help optimize your future NEET preparation, aiming for a higher All India Rank before the final exam.
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FAQs on Kinetic Theory Of Gases NEET Mock Test 3 (2025) – Free Online Practice
1. What is the kinetic theory of gases?
Kinetic theory of gases is a scientific model that explains the macroscopic properties of gases, such as pressure and temperature, based on the idea that gas molecules are in constant, random motion. It assumes that collisions between molecules and with the walls of the container are perfectly elastic and that the volume of individual gas molecules is negligible compared to the total volume of the container.
2. State the main assumptions of the kinetic molecular theory of gases.
The main assumptions of the kinetic molecular theory of gases are:
- Gas molecules are in continuous, random motion.
- The volume of gas molecules is negligible compared to the total gas volume.
- There are no intermolecular forces between gas molecules.
- Collisions between molecules and with container walls are perfectly elastic.
- The average kinetic energy of molecules is directly proportional to the absolute temperature.
3. Derive the expression for pressure exerted by an ideal gas using kinetic theory.
Using the kinetic theory of gases, the pressure (P) exerted by an ideal gas is derived as follows:
Consider a gas in a cubic container of volume V with N molecules of mass m and root mean square speed crms.
The pressure is given by: P = (1/3) ρ crms², where ρ is the mass per unit volume.
Thus, the relation shows that gas pressure is proportional to the average kinetic energy and density of molecules.
4. What is the relation between average kinetic energy and absolute temperature in the kinetic theory of gases?
The average kinetic energy of a gas molecule is directly proportional to its absolute temperature (T) and is given by the relation:
KEavg = (3/2) kB T,
where kB is Boltzmann constant. This means as temperature increases, the average kinetic energy of each molecule also increases.
5. What are the limitations of the kinetic theory of gases?
The main limitations of the kinetic theory of gases are:
- It assumes molecules have no size and do not exert any forces on each other, which is not true for real gases.
- The model is less accurate at high pressures and low temperatures.
- Cannot explain phenomena like condensation or deviations from ideal behavior (as seen in the Real Gas Law).
6. What is the difference between the kinetic theory of gases and the kinetic theory of radiation?
The kinetic theory of gases explains the physical properties of gases based on the movement of molecules, while the kinetic theory of radiation deals with the properties of radiant energy such as light, explaining it as a stream of particles (photons). While both theories use kinetic concepts, gases focus on matter and radiation on energy transmission.
7. Explain the concept of root mean square speed in kinetic theory.
The root mean square (rms) speed is a measure of the average speed of gas molecules. It is defined as the square root of the average of the squares of individual molecular speeds. For an ideal gas, it is given by:
crms = \( \sqrt{3RT/M} \),
where R is the gas constant, T is temperature, and M is the molar mass.
8. How is the pressure of a gas related to molecular motion according to kinetic theory?
According to kinetic theory, the pressure of a gas arises from the collisions of molecules with the walls of the container. Each collision transfers momentum to the wall, and the total effect of these collisions per unit time per unit area results in pressure.
9. Why do real gases deviate from ideal behavior?
Real gases deviate from ideal behavior because intermolecular forces become significant at high pressures or low temperatures, and the volume occupied by gas molecules cannot be neglected. The kinetic theory assumptions break down under such conditions, leading to observed deviations, which are better explained by the Van der Waals equation.
10. How does kinetic theory explain Boyle’s law and Charles’s law?
The kinetic theory of gases explains Boyle’s law (P ∝ 1/V at constant T) as the result of decreasing volume leading to more frequent collisions and higher pressure. Charles’s law (V ∝ T at constant P) is explained as an increase in temperature causing molecules to move faster, requiring more volume to maintain the same pressure.
11. What factors affect the rate of diffusion of a gas according to kinetic theory?
According to kinetic theory, the rate of diffusion of a gas depends on the following factors:
- Temperature: Higher temperature increases molecular speeds, raising diffusion rates.
- Molecular mass: Lighter gases diffuse faster than heavier ones (Graham’s law).
- Concentration gradient: Larger differences in concentration enhance diffusion rate.
12. How can practice with NEET mock tests on the kinetic theory of gases help improve exam performance?
Regular practice with NEET chapter-wise and full-length mock tests on topics like kinetic theory of gases helps aspirants by:
- Identifying weak areas and concepts that require revision.
- Improving speed and accuracy for MCQs.
- Familiarizing students with the exam pattern and time management.
- Providing instant feedback and detailed solutions for in-depth understanding and correction of mistakes.
