# Chemistry

In: Science

Submitted By smdionisio
Words 2245
Pages 9
I. INTRODUCTION Real gases are known to have non-ideal behavior characteristics because it does not exactly follow the ideal gas law. In the ideal gas law, gas molecules are considered to have negligible volume and negligible intermolecular interactions (Averill and Eldredge, 2006). The ideal gas equation of state is not sufficient to describe the pressure, volume and temperature behavior of most real gases but real gases shows significant deviations from the behavior of an ideal gas.

For real gases or non-ideal gases, the most common equation of states are shown below:
Van der Waals:
Berthelot:
Redlich-Kwong:
Dietirici:
Virial:

There are other equations of state that can be used to predict non-ideal gas behaviour and to incorporate a compression factor is another one. Compression factor, also known as compressibility factor is the ratio between molar volumes of a gas to the molar volume of a perfect gas. A perfect gas has a compression factor equal to 1 in all conditions so real gases deviates from that value.

Another equation for compression factor is

Fugacity is function of pressure and temperature

where Φ is the fugacity coefficient, a dimensionless quantity that depends on the temperature, pressure and identity of a gas. Getting Φ from the equation would result to the ratio of the fugacity and the effective pressure.
The fugacity coefficient approaches the value of 1 when the gas behaves like an ideal gas, so it is also a measure of non-ideality such as compression factor. The closer the value of the fugacity coefficient to 1, the closer it is for the gas to ideal behaviour. The compression factor, Z and fugacity coefficient,Φ, results to the given equation below by subjecting it to some substitution, integration and derivations.

This equation would be used to calculate Φ for...

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