A gas consisting of particles that could be atoms or
molecules is called an ideal gas if the particles that constitute the gas collide with
each other in a perfectly elastic manner. Also the particles should not have any
attractive forces between each other. If the gas can be pictured as one that is made up
of perfectly hard spheres with no inter particulate attraction it is called an ideal
gas. Internal energy in an ideal gas is purely kinetic, and a change in temperature is
accompanied by a proportional change in energy.
This can be
expressed by the relation PV= nRT perfectly. Here P is the pressure, V is the volume, n
is the number of moles, R is the universal gas constant and T is the temperature. Gases
around us are not ideal gases, so the ideal gas law is a close fit but does not exactly
express the properties of gases.
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