1. What is the Compressibility Factor?

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.

2. How Does the Calculator Work?

The calculator uses the compressibility factor equation:

Where:

• \( Z \) — Compressibility factor (dimensionless)
• \( P \) — Pressure (Pascals)
• \( V \) — Volume (cubic meters)
• \( n \) — Number of moles (moles)
• \( R \) — Universal gas constant (8.314462618 J/mol·K)
• \( T \) — Temperature (Kelvin)

Explanation: For an ideal gas, Z = 1. When Z < 1, attractive forces dominate; when Z > 1, repulsive forces dominate.

3. Importance of Compressibility Factor

Details: The compressibility factor is crucial in chemical engineering, thermodynamics, and petroleum engineering for accurate prediction of gas behavior under various conditions, especially at high pressures and low temperatures where gases deviate significantly from ideal behavior.

4. Using the Calculator

Tips: Enter pressure in Pascals, volume in cubic meters, number of moles, and temperature in Kelvin. All values must be positive and non-zero for accurate calculation.

5. Frequently Asked Questions (FAQ)

Q1: What does Z = 1 mean?
A: Z = 1 indicates ideal gas behavior where the gas follows the ideal gas law exactly.

Q2: When is Z typically less than 1?
A: Z < 1 usually occurs at moderate pressures where attractive intermolecular forces reduce the actual volume compared to an ideal gas.

Q3: When is Z typically greater than 1?
A: Z > 1 typically occurs at high pressures where repulsive intermolecular forces become significant, increasing the actual volume.

Q4: What is the range of Z values?
A: Z can range from near 0 (for highly compressed gases) to values greater than 2 (for light gases at high pressures).

Q5: How does temperature affect Z?
A: At constant pressure, Z generally increases with temperature as molecular motion increases and intermolecular forces become less significant.