What is not an assumption of the kinetic model of an ideal gas?
The statement, ‘At high pressure, gas particles are difficult to compress. ‘ is not an assumption of the kinetic theory of gases. In the postulates of the kinetic theory of gases, reference is made to low-pressure case but there is no reference to high-pressure case.
What can ideal gas not do?
Particles of a hypothetical ideal gas have no significant volume and do not attract or repel each other. In general, real gases approximate this behavior at relatively low pressures and high temperatures.
What are the assumptions of the kinetic model of an ideal gas?
The simplest kinetic model is based on the assumptions that: (1) the gas is composed of a large number of identical molecules moving in random directions, separated by distances that are large compared with their size; (2) the molecules undergo perfectly elastic collisions (no energy loss) with each other and with the …
Which of the following is not part of the kinetic molecular theory of gases?
Attractive and repulsive forces are present between gas molecule. According to the kinetic molecular theory, there is no attractive (or repulsive) force between the molecules, as they move independent of each other.
Which is not true in case of an ideal gas?
1 Answer. The correct option is : (c) All molecules of the gas move with same speed. Explanation: Molecules in an ideal gas move with different speeds.
Which of the following is not true about ideal gas molecules?
The option which is not true about ideal gas molecules is that they do not apply pressure (3rd option). The ideal gas is a hypothetical gas that is claimed to have all of the properties of the ideal gas law. There are no interparticle forces of attraction or repulsion amongst ideal gas molecules.
Why do real gases not behave like ideal gases?
The gas particles need to occupy zero volume and they need to exhibit no attractive forces whatsoever toward each other. Since neither of those conditions can be true, there is no such thing as an ideal gas. A real gas is a gas that does not behave according to the assumptions of the kinetic-molecular theory.
What are the limitations of kinetic theory of gases?
This fundamental equation of the kinetic theory of gases can be used to deduce various gas laws. The kinetic theory of gases has its limitations. This is clear from the behaviour of real gases which do not obey gas laws rigidly particularly at low temperatures and high pressures.
Why are intermolecular forces not effective in the gas phase of matter?
Intermolecular forces are weaker attractions that hold molecules or noble gas particles close together when they are in a liquid or solid form. Gas particles have broken away from the intermolecular forces that hold liquids and solids together.
Which one of the following gases would deviate the least from ideal gas behavior?
Neon has the smallest volume and least reactivity of all of the options, which means it would deviate the least from ideal gas behavior.
Which of the following is part of the kinetic molecular theory of gases?
The five main postulates of the KMT are as follows: (1) the particles in a gas are in constant, random motion, (2) the combined volume of the particles is negligible, (3) the particles exert no forces on one another, (4) any collisions between the particles are completely elastic, and (5) the average kinetic energy of …
Which of the following is true for an ideal gas?
EXPLANATION: Since the ideal gas molecules occupy negligible space, it can be concluded that they do not occupy space. The intermolecular forces between molecules of a matter are attractive in nature. As ideal gases do not have intermolecular forces, they do not have attractive forces between the molecules.