In Class 11 Final Exams there will be Case studies and Passage Based Questions will be asked, So practice these types of questions. Study Rate is always there to help you. Free PDF Downloads of CBSE Class 11 Physics Chapter 13 Case Study and Passage-Based Questions with Answers were Prepared Based on the Latest Exam Pattern. Students can solve Class 11 Physics Case Study Questions Kinetic Theory to know their preparation level.
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In CBSE Class 11 Physics Paper, There will be a few questions based on case studies and passage-based as well. In that, a paragraph will be given, and then the MCQ questions based on it will be asked.
Kinetic Theory Case Study Questions With Answers
Here, we have provided case-based/passage-based questions for Class 11 Physics Chapter 13 Kinetic Theory
Case Study/Passage-Based Questions
Case Study 1: Law of Equipartition of Energy – In equilibrium, the total energy is equally distributed in all possible energy modes, with each mode having average energy equal to (1/2) kT. This is known as the law of equipartition energy. Each translational and rotational degree of freedom contributes (1/2) kT to the energy. Each vibrational frequency contributes 2 × (1/2) kT = kT energy since vibration has both kinetic and potential modes of energy.
According to the equipartition law of energy, each particle in a system of particles have thermal energy E equal to
Answer: (d)
The average energy per molecule of a triatomic gas at room temperature T is
Answer: (a)
The gases carbon-monoxide (CO) and nitrogen are kept at the same temperature. If their kinetic energies are E1 and E2 respectively, then
(a) E1 = E2 (b) E1 > E2 (c) E1 < E2 (d) E1 and E2 cannot be compared
Answer: (a) E1 = E2
Which one of the following molecules does not possess vibrational energy?
(a) Oxygen (b) Nitrogen
(c) Argon (d) CO2
Answer: (c) Argon
Case Study 2: The kinetic theory of gases is a fundamental concept in physics that describes the behavior of gases based on the motion of their constituent particles. According to this theory, gases are composed of a large number of tiny particles, such as atoms or molecules, that are in constant random motion. The pressure exerted by a gas is a result of the collisions between these particles and the walls of the container. The kinetic energy of the gas particles is directly proportional to their temperature, and as the temperature increases, the particles move with higher velocities, resulting in an increase in pressure. The kinetic theory also explains the relationship between temperature and the average kinetic energy of the gas particles. At the same temperature, all gases have an equal average kinetic energy per molecule. This theory has been essential in understanding various gas properties and phenomena, including diffusion, effusion, and the ideal gas law.
The kinetic theory of gases describes the behavior of gases based on the motion of their constituent particles, which are:
(a) Constantly at rest
(b) In constant random motion
(c) Arranged in a regular pattern
(d) Composed of protons and electrons
Answer:(b) In constant random motion
The pressure exerted by a gas is a result of the collisions between gas particles and:
(a) The walls of the container
(b) Each other
(c) The surrounding atmosphere
(d) The gravitational force
Answer: (a) The walls of the container
The kinetic energy of gas particles is directly proportional to their:
(a) Mass
(b) Temperature
(c) Volume
(d) Pressure
Answer: (b) Temperature
According to the kinetic theory, at the same temperature, all gases have an equal average kinetic energy per:
(a) Molecule
(b) Atom
(c) Gram
(d) Liter
Answer: (a) Molecule
Case Study 3:
The pressure of an Ideal Gas: according to the kinetic theory of gases pressure is given by
P = 1/3 nmv2
Where n is a number of molecules per unit volume, m is mass and v2 is the mean squared speed. Though we choose the container to be a cube, the shape of the vessel really is immaterial.
The average kinetic energy of a molecule is proportional to the absolute temperature of the gas; it is independent of pressure, volume, or the nature of the ideal gas. This is a fundamental result relating temperature, a macroscopic measurable parameter of a gas (a thermodynamic variable as it is called) to a molecular quantity, namely the average kinetic energy of a molecule. The two domains are connected by the Boltzmann constant and given by E = kbT.
Where kb is Boltzmann constant having a value of 1.38*10-23 joule per Kelvin.
We have seen that in thermal equilibrium at absolute temperature T, for each translational mode of motion, the average energy is ½ Kb T. The most elegant principle of classical statistical mechanics (first proved by Maxwell) states that this is so for each mode of energy: translational, rotational, and vibrational. That is, in equilibrium, the total energy is equally distributed in all possible energy modes, with each mode having an average energy equal to ½ kB T. This is known as the law of equipartition of energy. Accordingly, each translational and rotational degree of freedom of a molecule contributes ½ kB T to the energy, while each vibrational frequency contributes 2 × ½ kB T = kB T since a vibrational mode has both kinetic and potential energy modes.
According to the kinetic theory of gases, what is the relationship between pressure (P) and the number of molecules per unit volume (n), mass (m), and mean squared speed (v^2)?
a) P = 1/2 nmv^2
b) P = 1/3 nmv^2
c) P = 2/3 nmv^2
d) P = 3/2 nmv^2
Answer: b) P = 1/3 nmv^2
What does the average kinetic energy of a molecule in an ideal gas depend on?
a) The pressure and volume of the gas
b) The absolute temperature of the gas
c) The nature of the gas
d) The size of the container
Answer: b) The absolute temperature of the gas
How is the Boltzmann constant denoted, and what is its value?
a) kB, 1.38 x 10-23 joule per Kelvin
b) k, 1.38 x 10-22 joule per Kelvin
c) B, 1.38 x 10-24 joule per Kelvin
d) kB, 1.38 x 10-20 joule per Kelvin
Answer: a) kB, 1.38 x 10-23 joule per Kelvin
The law of equipartition of energy states that the total energy is equally distributed in all possible energy modes. This principle was first proved by whom?
a) Boltzmann
b) Maxwell
c) Planck
d) Einstein
Answer: b) Maxwell
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