Regarding the compressibility factor
Thread Content
The larger the compressibility factor of a gas, is it easier to compress it, or smaller? I always get it mixed up~
For an ideal gas, Z = 1; for real gases, Z can be greater than, less than, or equal to 1. Therefore, the extent to which Z deviates from 1 indicates the degree to which it deviates from an ideal gas. Under normal conditions, Z varies with the pressure and temperature of the gas. For an ideal gas, Z is always equal to 1 at any temperature and pressure. When Z is less than 1, it indicates that the molar volume of a real gas is larger than that of an ideal gas under the same conditions; in such cases, the real gas is more difficult to compress than an ideal gas.
The definition of the compression factor is not based on the compressed volume; it has no relation to the compression of gases.
A low pressure is sufficient to achieve a small volume after compression...
The compressibility factor is a measure of how much a real gas differs from an ideal gas; it is given by Z = pV/nRT = V(real)/V(ideal), and its ease of compression is also a relative concept with respect to ideal gases
For an ideal gas, Z=1, and it can be calculated using the SRK and PR equations
Compressibility factor Z = PV/nRT = V(true)/V(theoretical) Z