Assertion (A): Real gases tend to behave as ideal gas at low pressure and high Temperature.
Reason (R): At temperature more than critical temperature, a gas can’t be liquefied just by increasing the pressure. Which of the followings is correct?
Assertion (A): Real gases tend to behave as ideal gas at low pressure and high Temperature.
Reason (R): At temperature more than critical temperature, a gas can’t be liquefied just by increasing the pressure. Which of the followings is correct?
The correct option is B Both A and R are true but R is not a correct explanation of A.
According to kinetic theory of gases, ideal gases have no attractive force between their molecules. The volume occupied by the gas molecules themselves is also considered to be zero. Both these conditions are not true for real gases at normal pressure and temperature. But at low pressure and high temperature, molecules are widely spread and kinetic energy of molecules is very high. These conditions make intermolecular forces negligible. The volume occupied by the molecules themselves is also negligible compared to the volume occupied by the gas. Hence real gas tends to behave as an ideal gas at low pressure and high temperature. Thus A is true.
‘R’ is the definition of critical temperature, hence it is true.
According to kinetic theory of gases, ideal gases have no attractive force between their molecules. The volume occupied by the gas molecules themselves is also considered to be zero. Both these conditions are not true for real gases at normal pressure and temperature. But at low pressure and high temperature, molecules are widely spread and kinetic energy of molecules is very high. These conditions make intermolecular forces negligible. The volume occupied by the molecules themselves is also negligible compared to the volume occupied by the gas. Hence real gas tends to behave as an ideal gas at low pressure and high temperature. Thus A is true.
‘R’ is the definition of critical temperature, hence it is true.
