The critical temperature `(T_(c))` and critical pressure `(p_(c))` of `CO_(2)` are `30.98^(@)C` and 73 atm respectively. Can `CO_(2) (g)` be liquefied at `32^(@)C` and 80 atm pressure ?

Critical temperature (T_(C)) and critical pressure (P_(C)) of carbon dioxide gas are 30.98^(@) C and 73 atm . Carbon dioxide gas cannot be liquified under following conditions

Calculate van der Waals constansts a and b if critical temperature and critical pressure are 30^(@)C and 72 atm respectively .

Calculate van der Waals constansts a and b if critical temperature and critical pressure are 30^(@)C and 72 atm respectively .

A real gas has critical temperature and critical pressure as 40^(@)C and 10 atm respectively, then liquification of gas is possible at

A real gas has critical temperature and critical pressure as 40^(@)C and 10 atm respectively, then liquification of gas is possible at

What is the density of CO_(2) at 27 .^(@)C and 2.5 atm pressure ?

What is the density of CO_(2) at 27 .^(@)C and 2.5 atm pressure ?

The critical temperature and the critical pressure of a gas are T_(c) and P_(c) , respectively. If the gas exists at a temperature of T and a pressure P, then under which of the following conditions will the gas not be liquefied? (i) T gt T_(c) , P gt P_(c) (ii) T=T_(c),PgtP_(c) (iii) T=T_(c),PltP_(c) (iv) T lt T_(c),P=P_(c)