Proven Strategies to Score High in JEE Main Kinetic Theory Of Gases Mock Tests
Kinetic Theory of Gases is a foundational chapter for JEE Physics, diving into the behavior of gas molecules, their collisions, and how microscopic motion explains macroscopic properties. This mock test will help you master essential laws, formulas, and concepts like pressure, RMS speed, and energy distribution—crucial for acing JEE Main. Take this test now to strengthen your problem-solving skills and boost your exam confidence!
Mock Test Instructions for the Kinetic Theory Of Gases Mock test-3:
- 20 questions from Kinetic Theory Of Gases Mock test-3
- 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 Kinetic Theory of Gases?
- Identify and overcome common conceptual errors regarding molecular collisions and assumptions.
- Repeatedly practice MCQs on kinetic energy, Maxwell’s distribution, and pressure calculations to boost recall.
- Strengthen problem-solving speed in RMS, average, and most probable speed calculations under exam timing.
- Assess and improve your application of kinetic theory postulates with instant feedback from test analytics.
- Discover tricky areas in real JEE questions involving gas laws, molecular velocities, and temperature effects.
Master Gas Laws and Molecular Motion with Expert-Designed JEE Chapter Mock Tests
- Test your command on formulas linking molecular speed, temperature, and pressure, curated for JEE standards.
- Work on previous year patterns with time-bound mock tests reflecting NTA’s latest exam structure.
- Practice application-based problems for pressure, energy distribution, and Maxwell’s law with guided explanations.
- Build exam confidence by identifying weak zones in KTG and tackling them with focused mock practice.
- Enhance your retention of essentials like Avogadro's number, Boltzmann constant, and SI units for KTG.
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FAQs on JEE Main 2025-26: Kinetic Theory Of Gases Mock Test for Effective Preparation
1. What is the kinetic theory of gases?
Kinetic theory of gases is a scientific model that explains the behavior and properties of gases based on the assumption that gases consist of a large number of small particles (molecules or atoms) moving in random directions with high speeds. It states that gas pressure arises from the collisions of these molecules with the walls of the container. The theory helps derive relationships such as the ideal gas equation and connects microscopic behavior with macroscopic observations like temperature and pressure.
2. State the main postulates of the kinetic molecular theory of gases.
The main postulates of the kinetic molecular theory of gases are:
1. Gases are composed of a large number of tiny particles that are in constant, random motion.
2. The volume of individual gas molecules is negligible compared to the total volume of the gas.
3. There are no forces of attraction or repulsion between the gas molecules.
4. Collisions between gas particles and with the container walls are perfectly elastic.
5. The average kinetic energy of the gas molecules is directly proportional to the absolute temperature of the gas.
3. What is the relationship between temperature and average kinetic energy of gas molecules?
According to the kinetic theory of gases, the average kinetic energy of gas molecules is directly proportional to the absolute (Kelvin) temperature of the gas. Mathematically: Average kinetic energy = (3/2)kT, where k is Boltzmann's constant and T is temperature in Kelvin.
4. Define the term mean free path.
The mean free path is the average distance traveled by a gas molecule between two consecutive collisions with other molecules. It depends on the number density of molecules and their diameter. A higher pressure or more crowded container leads to a shorter mean free path.
5. Explain the concept of root mean square (RMS) velocity.
Root mean square (RMS) velocity is the square root of the average of the squares of the individual velocities of gas molecules. It is given by the formula: vrms = √(3RT/M), where R is the gas constant, T is absolute temperature, and M is the molar mass. RMS velocity helps in understanding the energy and speed distribution among gas molecules.
6. What assumptions are made in the kinetic theory of gases while deriving the ideal gas equation?
The kinetic theory of gases assumes:
1. Gas molecules are point masses with negligible volume.
2. There are no intermolecular attractions or repulsions.
3. Collisions are perfectly elastic.
4. Gases consist of many molecules moving randomly.
5. The time taken for a collision is negligible compared to the time between collisions.
These assumptions are valid for ideal gases under moderate temperature and low pressure.
7. What is the difference between diffusion and effusion of gases?
Diffusion is the process by which gas molecules mix with each other due to their random motion, spreading uniformly throughout the available volume. Effusion is the movement of gas molecules through a small opening or a porous barrier from an area of higher pressure to lower pressure. Both are explained using the kinetic molecular theory.
8. How does kinetic theory explain the pressure of a gas?
The kinetic theory of gases explains that pressure is caused by the continuous collisions of gas molecules with the walls of the container. Each collision exerts a force, and the total effect of all these collisions over a surface area results in the observed gas pressure. Higher temperature or more frequent/harder collisions increase the pressure.
9. What are the limitations of the kinetic theory of gases?
The main limitations of the kinetic molecular theory are:
1. It assumes there are no intermolecular forces, which is not true for real gases, especially at high pressure or low temperature.
2. It neglects the finite volume of gas molecules.
3. It assumes perfectly elastic collisions and uniform molecular motion, which may not always apply.
Because of these assumptions, the theory applies best to ideal gases under standard conditions.
10. What is black body radiation?
Black body radiation is the electromagnetic radiation emitted by a body that absorbs all incident radiation, regardless of wavelength. A perfect black body does not reflect or transmit any energy, and its emission depends only on its temperature. This concept is vital in radiation physics and helped lead to the development of quantum mechanics.
11. State the laws of black body radiation.
The important laws of black body radiation are:
1. Planck's Law: Describes the intensity of radiation emitted at different wavelengths by a black body at a given temperature.
2. Stefan-Boltzmann Law: The total energy radiated per unit surface area is directly proportional to the fourth power of absolute temperature (E ∝ T4).
3. Wien's Displacement Law: The wavelength at which the emission is maximum is inversely proportional to the absolute temperature (λmax ∝ 1/T).
12. What is the Maxwell distribution of molecular speeds?
The Maxwell distribution describes the probability distribution of speeds among molecules in a gas. It shows that molecules have a wide range of speeds, but most are near an average value (most probable speed). The distribution changes with temperature, becoming broader and shifted towards higher speeds as temperature increases.
