Question

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 compressibility factor $Z$ and pressure $P$.
What is the deviation of real gas from ideal behaviour in terms of compressibility factor, $Z$?

• A. As the temperature increases, $Z$ approaches a value close to one and gas starts behaving ideally
• B. $Z$ continuously decrease with increase in pressure
• C. $Z$ continuously increase with increase in pressure
• D. At high pressure, every gas has value $Z=1$

Answer 1

The correct option is A As the temperature increases, $Z$ approaches a value close to one and gas starts behaving ideally

Compressibility factor Z is a correction factor which gives the deviation of a real gas from an ideal gas. It is the ratio of the molar volume of a gas to the molar volume of an ideal gas, at same T and P. Here as the temperature increases, Z starts approaching towards one and then the gas starts behaving ideally.