Statement 1: At Boyle temperature, the compressibility factor of a real gas, Z ≥ 1.
Statement 2: All the gases tend to approach a value Z = 1, when the pressure of gas approaches to zero value at any temperature.

Question

Statement 1: At Boyle temperature, the compressibility factor of a real gas, Z ≥ 1.

Statement 2: All the gases tend to approach a value Z = 1, when the pressure of gas approaches to zero value at any temperature.

TestHub · Accepted Answer

Statement 1 is correct: in the virial form Z = 1 + B 2 (T)(P/RT) + B 3 (T)(P/RT) 2 + cdots, the Boyle temperature is defined by B 2 = 0 while the higher coefficients are positive, so at T B we get Z = 1 in the zero-pressure limit and Z > 1 at any finite pressure, i.e. Z ≥ 1 everywhere. Statement 2 is also correct (Z → 1 as P → 0 at any T), but it is a statement about the low-pressure limit at all temperatures, not the reason Z ≥ 1 holds specifically at T B . Both correct, II not the explanation. Ans: (b).

Chemistry - Real Gas Question with Solution | TestHub

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