Introduction - Gaseous State, Liquid State, Solid State

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Introduction

In order to experimentally determine the properties of substances, we deal with the aggregates of molecules as they occur in nature. It is the aggregations of molecules which come within the scope of human experience that constitute what is known as matter. The various kinds of substances that make up matter can be divided roughly into three categories, namely gases, liquids, and solids. These are called the three states of matter. These states can be considered to arise as a result of competition between two opposing molecular forces, namely, the forces of attraction which tend to hold the molecules together, and the disruptive forces dut to the thermal energy of molecules.
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Gaseous State

If the thermal energy is much greater than the forces of attraction, then we have matter in its gaseous state. Molecules in the gaseous state move with very large speeds and the forces of attraction amongst them are not sufficient to bind the molecules at one place, with the result that the molecules move partially independent of one another. Because of this feature, gases are characterized by marked sensitivity of volume change with a change in temperature and pressure. There exists no boundary surface and, therefore, gases than to fill completely any available space, resulting in no fixed volume to the gaseous state.
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Liquid State

If the forces of attraction are greater than the thermal energy, we have matter in the liquid state. Molecules in the liquid state to have kinetic energy but they cannot go very far away because of the larger forces of attraction amongst them. Due to this feature, liquids have a definite volume, but no definite shape. They take the shape of the vessel in which they are placed. In general, liquids are denser and less compressible than gases.

Solid State

If the forces of attraction between molecules are much greater than the thermal energy, the positions of the molecules remain fixed and we have matter in the solid-state. The molecules in the solid-state, therefore, do not possess any translational energy but have only vibrational energy since they can vibrate about their mean positions. Extremely large forces of attraction exist amongst them. That is way solids differ markedly from liquids and gases in respect of size, shape volume. Solids, in general, have definite size, shape, and volume.

Comments on the Gaseous System

Of all the three states of molecular aggregation, only the gaseous state allows a comparatively simple quantitative description. We are generally concerned with the relations among four properties, namely, mass, pressure, volume, and temperature. A system is in a definite state (or condition) when all the properties of the system have definite values. It is not necessary to specify each and every property of the matter as these are interrelated. The relationship which connects the above four variables is known as the equation of state of the system. For gases, only three of these must be specified to describe the state, the fourth automatically has a fixed value and can be calculated from the equation of state established from the experimental behavior of the system.
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