Question

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a sample of o2 gas initially at stp is transferred from 1 litre container to 2 litre container at a constant temperature then
(a) the average kinetic energy of the molecule will decrease
(b) the total number of collisions of o2 molecules with container wall will decrease. the pressure of the gas will increase
(c) the pressure of gas will decrease
(d) rms speed of molecule will remain unchainged

Answer 1

Answer:

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The Kinetic-Molecular Theory

LEARNING OBJECTIVES

By the end of this section, you will be able to:

State the postulates of the kinetic-molecular theory

Use this theory’s postulates to explain the gas laws

The gas laws that we have seen to this point, as well as the ideal gas equation, are empirical, that is, they have been derived from experimental observations. The mathematical forms of these laws closely describe the macroscopic behavior of most gases at pressures less than about 1 or 2 atm. Although the gas laws describe relationships that have been verified by many experiments, they do not tell us why gases follow these relationships.

The kinetic molecular theory (KMT) is a simple microscopic model that effectively explains the gas laws described in previous modules of this chapter. This theory is based on the following five postulates described here. (Note: The term “molecule” will be used to refer to the individual chemical species that compose the gas, although some gases are composed of atomic species, for example, the noble gases.)

Gases are composed of molecules that are in continuous motion, travelling in straight lines and changing direction only when they collide with other molecules or with the walls of a container.

The molecules composing the gas are negligibly small compared to the distances between them.

The pressure exerted by a gas in a container results from collisions between the gas molecules and the container walls.

Gas molecules exert no attractive or repulsive forces on each other or the container walls; therefore, their collisions are elastic (do not involve a loss of energy).

The average kinetic energy of the gas molecules is proportional to the kelvin temperature of the gas.

The test of the KMT and its postulates is its ability to explain and describe the behavior of a gas. The various gas laws can be derived from the assumptions of the KMT, which have led chemists to believe that the assumptions of the theory accurately represent the properties of gas molecules. We will first look at the individual gas laws (Boyle’s, Charles’s, Amontons’s, Avogadro’s, and Dalton’s laws) conceptually to see how the KMT explains them. Then, we will more carefully consider the relationships between molecular masses, speeds, and kinetic energies with temperature, and explain Graham’s law.

Answer 2

Answer:

The answer is  actually both the options A &B

(a) the average kinetic energy of the molecule will decrease.

(b) the total number of collisions of o2 molecules with container wall will decrease. the pressure of the gas will increase.

Explanation:

I f a gas is transferred from a small container into a larger container

then,Gas particles would spread to the full size of the larger container.

The Kinetic Molecular Theory of gases

          The kinetic molecular theory provides a straightforward theoretical framework that can be used to explain the experimental results concerning the behaviour of gases mentioned thus far. The following premises, or postulates, form the foundation of this theory.

• Gases are composed of a large number of particles that behave like hard, spherical objects in a state of constant, random motion.
• These particles move in a straight line until they collide with another particle or the walls of the container.
• These particles are much smaller than the distance between particles. Most of the volume of a gas is therefore empty space.
• There is no force of attraction between gas particles or between the particles and the walls of the container.
• Collisions between gas particles or collisions with the walls of the container are perfectly elastic. None of the energy of a gas particle is lost when it collides with another particle or with the walls of the container.
• The average kinetic energy of a collection of gas particles depends on the temperature of the gas and nothing else.

• Any object in motion has a kinetic energy that is defined as one-half of the product of its mass times its velocity squared.

                              KE = 1/2 mv2

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