Measurable Properties of Gases

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 …

1)Every gas is made up of a large number of extremely small particles called molecules. 3)The distance of separation between the molecules are so large that the forces of attraction or repulsion between them are negligible. 4)The force of gravitation on the molecule is also supposed to be negligible.

• (1) The characteristics of gases are described fully in terms of four parameters or measurable properties:
• (i) The volume, V, of the gas.
• (ii) Its pressure, P.
• (iii) Its temperature, T.
• (iv) The amount of the gas (i.e., mass or number of moles).

As applied to gases, the kinetic molecular theory has the following postulates: Gases are composed of very tiny particles (molecules). The actual volume of these molecules is so small as to be negligible compared with the total volume of the gas sample. A gas sample is, then, mostly empty space.

The kinetic-molecular theory of gases can be stated as four postulates:

• A gas consists of molecules in constant random motion.
• Gas molecules influence each other only by collision; they exert no other forces on each other.
• All collisions between gas molecules are perfectly elastic; all kinetic energy is conserved.

What is a postulate of the kinetic molecular theory of gases? The particles that compose a gas are so small compared to the distances between them that the volume of the individual particles can be assumed to be negligible.

Terms in this set (5)

• Gases are composed of infinitely small particles.
• The volume of a gas is composed of the space between the particles.
• Particles are in a constant random motion.
• Particles do not gain or lose kinetic energy during collision.
• Average kinetic energy of the particles is proportioned to temperature.

Five Postulates of KMT. Gas particles have negligible volume compared to the free space between them.. Molecular collisions are perfectly elastic and kinetic energy is conserved. Gas particles experience negligible intermolecular forces, there are no attractive or repulsive forces between particles.

Which postulate of the kinetic-molecular theory best describes the event in the diagram? All collisions between particles are perfectly elastic.

A limitation of the kinetic-molecular theory for a gas is the theory assumes that particles do not experience intermolecular forces. This cannot be completely true since interactions between particles is normal.

The two conditions that can limit the usefulness of the kinetic-molecular theory in describing gas behavior are “high pressure” and “low temperatures”.

Which statement describes a limitation of the kinetic-molecular theory for a gas? The theory assumes that particles do not experience intermolecular forces. The theory states that pressure is inversely proportional to volume. The theory assumes that particles are in random and continuous motion.

If the average kinetic energy is greater than the attractive forces between the particles, a substance will not condense to form a liquid or a solid. If the kinetic energy is less than the attractive forces, a liquid or solid will form.

Water is known to be the universal solvent because it can mostly dissolve most of the substances. The reason behind its solvability is the bonding of intermolecular forces of attraction. The answer is letter B. Out of the many bondings between molecules, the bond that governs water is H bonding or hydrogen bonding.