The compressibility factor of a real gas is given by . At temperatures significantly above the Boyle temperature (), what is the typical behavior of as pressure increases from zero?

Question

The compressibility factor $Z$ of a real gas is given by $Z = PV/nRT$. At temperatures significantly above the Boyle temperature ($T > T_B$), what is the typical behavior of $Z$ as pressure increases from zero?

Prashant Kotian · Accepted Answer

Correct answer: D. Above the Boyle temperature, thermal energy dominates over attractive forces. Consequently, the effect of molecular size (repulsion) is the only significant deviation, causing to be strictly greater than and increase steadily with pressure ().

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