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Compressibility Factor Equation:
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The compressibility factor (z) is a dimensionless quantity that describes the deviation of a real gas from ideal gas behavior. It is defined as the ratio of the actual molar volume of a gas to the molar volume of an ideal gas at the same temperature and pressure.
The calculator uses the compressibility factor equation:
Where:
Explanation: For an ideal gas, z = 1. For real gases, z deviates from 1 due to intermolecular forces and finite molecular size.
Details: The compressibility factor is crucial in thermodynamics and chemical engineering for accurate prediction of gas behavior under various conditions, particularly in high-pressure applications where gases deviate significantly from ideal behavior.
Tips: Enter pressure in pascals, volume in cubic meters, amount of substance in moles, gas constant in J/mol K, and temperature in kelvin. All values must be positive.
Q1: What does z = 1 indicate?
A: z = 1 indicates ideal gas behavior where the gas follows the ideal gas law perfectly.
Q2: When is z greater than 1?
A: z > 1 typically occurs at high pressures where repulsive forces between molecules dominate, making the gas less compressible than an ideal gas.
Q3: When is z less than 1?
A: z < 1 typically occurs at moderate pressures where attractive forces between molecules dominate, making the gas more compressible than an ideal gas.
Q4: What is the typical range of z values?
A: For most gases under common conditions, z ranges from about 0.2 to 2.0, though extreme conditions can produce values outside this range.
Q5: How does temperature affect z?
A: At constant pressure, z generally approaches 1 as temperature increases, since higher temperatures reduce the effects of intermolecular forces.