What is the ideal gas?
Ideal gas is a theoretical condition that physics use probability theory analysis. The ideal gas consists of molecules that are discouraged without otherwise interacting. There are no attraction or repeling forces among molecules and no energy is lost during the collision. The ideal gases can be completely described according to their volume, density and temperature.
The state equation for ideal gas, commonly known as the ideal gas law, is PV = NKT. In the equation there is n number of molecules and K is the Boltzmann constant, which is equal to 1.4 x 10 -23 joules on Kelvin. It is usually more important that pressure and volume are inversely proportional and each is proportional to the temperature. For example, this means that if the pressure is doubled, while the temperature is kept constant, then the gas volume must be half; If the gas volume doubles when the pressure is maintained constant, the temperature must also double. Institute of examples are considered constant in gas.
Of course, it is only approximation. The precipitation between gas molecules is not perfectly elastic, some energy and there are electrostatic forces between gas molecules. In most everyday situations, however, the Act on Ideal Gas closely closer to the real behavior of gases. Although not used to perform calculations, maintaining the relationships between pressure, volume and temperature can help the scientist understand the behavior of gas intuitively.
The ideal gas Act is often the first equation that people learn to study gases in the opening physics or chemical class. The Van der Waal equation, which includes several minor repairs of the basic prerequisites of the Act on the Ideal Gas, is also taught in many introductory courses. In practice, however, correction is so small that if the ideal gas is not sufficiently accurate for the application, the Van der Waal equation will not be good enough.
As with most thermodynamics, it is also assumed that idealGas is in a state of balance. This assumption is obviously false if the pressure, volume or temperature changes; If these variables change slowly, a state called a static equilibrium, but the error may be acceptably small. Giving up the assumption of a quasi of static balance means leaving thermodynamics behind for a more complicated world of statistical physics.