Explain the significance of critical temperature and critical pressure for `CO_2` which is kept at `31.10^@C`. A minimum pressure of 72.9 atm should be applied to liquify it.

Critical temperature of some substance are given below: It is not possible to liquify CO_2 gas above 31.1^@C by applying pressure. Why ?

The critical temperature and pressure of CO_(2) gas are 304.2 K and 72.9 atm respectively. What is the radius of CO_(2) molecule assuming it to behave as vander Waal's gas

Calculate the pressure exerted by 4.4 g of CO_2 gas which is kept in a 1 litre flask at 0^circ C .

The Henry's law constant for 02 dissolved in water is 4.34 xx 10^(4) atm at certain temperature. If the partial pressure of O_(2) in a gas mixture that is equilibrium with water is 0.434 atm, what is the mole fraction of O_(2) in the solution?

The critical temperatures of ammonia and carbon dioxide are 405.5K and 304.10 K respectively. On cooling, which of these gases will liquify first? Justify.

The gases which obey Gas Laws at all temperatures and pressures are called ideal gases. Calculate the minimum pressure required to compress 500mL of air at 1 atm to 300mL at the same temperature.