The vander waals constant for `O_(2)` are a = 1.36 atm `L^(2) mol^(-2) ` and `b = 0.0318 L mol^(-1)`. Calculate the temperature at which `O_(2)` gas behaves, ideally for longer range of pressure.

The van der Waal's constants for a gas are a=1.92 atm L^(2) "mol"^(-2),b=0.06 L "mol"^(-1) . If R = 0.08 L atm K^(-1) "mol"^(-1) , what is the Boyle's temperature (in K) of this gas ?

If the Vander Waal's constant of gas A are given as - a ( atm L^(2) mol^(2) ) =6.5 b( L mol^(1) ) 0.056 than critical pressure of A is

Given that the co-volume of O_(2) gas is 0.318 L mol^(-1) . Calculate the radius of O_(2) molecule.

Calculate the pressure exerted by 110 g of carbon dioxide in a vessel of 2 L capacity at 37^(@)C . Given that the van der Waal’s constants are a = 3.59 L^(2) " atm "mol^(-2) and b = 0.0427 L mol^(-1) . Compare the value with the calculated value if the gas were considered as ideal.

Calculate the pressure exerted by 110 g of carbon dioxide in a vessel of 2 L capacity at 37^(@)C . Given that the van der Waal’s constants are a = 3.59 L^(2) " atm "mol^(-2) and b = 0.0427 L mol^(-1) . Compare the value with the calculated value if the gas were considered as ideal.