Question

What is Boyle temperature?

Answer 1

As we know that a real gas which obey gas law at high temperature and low pressure. But a real gas shows maximum deviation from gas law at low temperature and high pressure and as the temperature increases, the real gas starts behaving as an ideal gas.

Complete step by step answer:
As we are well aware of the fact that a real gas is the one that obeys gas law at conditions of high pressure and low temperature. But when real gases show maximum deviation from gas law they start behaving as ideal gases following the conditions of low temperature and high pressure.
So, we can say that at a particular temperature, the real gases starts behaving as ideal gases and this particular temperature is known as Boyle’s temperature which is given as:
${T_b} = \dfrac{a}{{Rb}}$
Where $a$ and $b$ are the Van der waals constants and $R$ is the universal gas constant.
This also means that at a particular temperature the value of compressibility factor which is represented as $Z$ reaches to $1$ at a low pressure range. The compressibility factor is given as:
$Z = \dfrac{{P{V_m}}}{{RT}}$
where pressure and volume are directly related and temperature is inversely related to the compressibility factor. And for an ideal gas the value of compressibility factor is one.
For a real gas, the attractive forces and the repulsive forces acting on the particular gas arrives at a balance at Boyle’s temperature.

Note: Always remember that Boyle's temperature is different from the critical temperature because critical temperature is that particular temperature on which a gas starts behaving as a non-ideal gas and it is always lower than that of Boyle’s temperature.