Explanation
The compressibility factor (Z), also known as the compression factor, is the ratio of the molar volume of a gas to the molar volume of an ideal gas at the same temperature and pressure for an ideal gas the compressibility factor is 1.
The intermolecular forces operating amongst gas molecules vary with temperature and pressure. In fact, deviations from ideality occur due to both attractive and repulsive forces. The Kinetic Gas theory makes two controversial assumptions: 1.Gas molecules are point sized particles occupying negligible volume 2. They exert negligible forces on each other. The Boyle temperature is the temperature at which, intermolecular forces among gas molecules are minimized. As we go towards relatively lower temperatures and higher pressures, both the above assumptions fail. Gas molecules occupy a considerable part of the container volume, and attractive forces begin to dominate. As a result, the impact of the molecules on the container walls is reduced; thereby pressure falls less than the 'ideal' value. Contrastingly, at high temperatures, repulsive forces begin to dominate; pressure becomes higher than the 'ideal' value.
According to Boyle’s law, p ∝ 1/V , Hence in order to increase the volume of a gas by 10% , the pressure of the gas should be decreased be 10 % .
Daltons law of partial pressure is applicable only for non-reacting gases. According to this law, p = p1 + p2 + p3 +………
Where , p1, p2, p3,…. are partial pressures of components of gases.
Consider the following systems,
Isothermal process taking place in a thermodyanmics system at constant temperature and adiabatic process taking place in a thermodynamic system for which there is no exchange of heat between the system and its surroundings. In both the process, the temperature is same or constant and these two process obeyes Boyle’s law at constant temperature.
Therefore ideal gas equation pV = nRT is obeyed by ideal gas in both isothermal and adiabatic process.
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