Boyle’s temperature or Boyle point is the temperature at which a real gas starts behaving like an ideal gas over a particular range of pressure. A graph is plotted between the compressibility factor Z and pressure P. What is the variation of Z with P?

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At very low pressures, all gases show Z=1

At high pressures, all gases show Z>1

At intermediate pressures, all gases show Z<1

All of the above

answer is D.

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Detailed Solution

Concept: Since it influences how far real gases deviate from ideal behaviour, compressibility factor is a crucial factor in real gases. Z stands for it. It is displayed in two ways: pressure variation at constant temperature and pressure variation at various temperatures.
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At very low pressure, all gases show negative deviation from ideal behaviour. so, Z=1
At high pressure, all gases show a positive deviation for ideal behaviour. So, the value of Z > 1.
At intermediate pressure, the value is Z < 1, due to negative deviation.
Only methane and carbon monoxide exhibit Z<1 for specific pressure ranges. For all pressure values, all other gases have a Z>1 value. A gas behaves more like an ideal gas as its temperature rises because the intermolecular forces of attraction weaken more and more when heat is added to the system.
Hence, the correct answer is option 4.

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