therefore have no forces of attraction between them. The gas particles are also in a state of constant motion, with a high velocity and kinetic energy. In reality, there are forces of attraction present between the gas particles, but the high kinetic energy and the resultant motion of the gas particles does not allow these forces to manifest themselves. However, going from gas to liquid to solid, molecular separation and particle velocities reduce, resulting in an increase in the attractive forces. The stronger intermolecular forces will be able to draw molecules together, resulting in a condensed phase (solid or liquid). These intermolecular forces are also responsible for other properties like the viscosity of liquids and surface tension in solids. 1. a.Draw labelled representations of H2 in the solid, liquid and gas phases b. Draw labelled representations of He in the solid, liquid and gas phases she boxCidentiv 2. In which physical state(s) are the attractions between individual particles (atoms or molecules) stronger?
Ideal and Real Gases
Ideal gases obey conditions of the general gas laws under all states of pressure and temperature. Ideal gases are also named perfect gases. The attributes of ideal gases are as follows,
Gas Laws
Gas laws describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. The very first observations about the physical properties of gases was made by Robert Boyle in 1662. Later discoveries were made by Charles, Gay-Lussac, Avogadro, and others. Eventually, these observations were combined to produce the ideal gas law.
Gaseous State
It is well known that matter exists in different forms in our surroundings. There are five known states of matter, such as solids, gases, liquids, plasma and Bose-Einstein condensate. The last two are known newly in the recent days. Thus, the detailed forms of matter studied are solids, gases and liquids. The best example of a substance that is present in different states is water. It is solid ice, gaseous vapor or steam and liquid water depending on the temperature and pressure conditions. This is due to the difference in the intermolecular forces and distances. The occurrence of three different phases is due to the difference in the two major forces, the force which tends to tightly hold molecules i.e., forces of attraction and the disruptive forces obtained from the thermal energy of molecules.
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