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 ?

The van der Waals' constantes for a gas are a=3.6 atmL^(2)mol^(-2),b=0.6Lmol^(-1) .If R=0.08LatmK^(-1)mol^(-1) and the Boyle's temperature (K) is T_(B) of this gas, then what is the value of (T_(B))/(15) ?

The van der Waals' constantes for a gas are a=3.6 atmL^(2)mol^(-2),b=0.6Lmol^(-1) .If R=0.08LatmK^(-1)mol^(-1) and the Boyle's temperature (K) is T_(B) of this gas, then what is the value of (T_(B))/(15) ?

The van der Waals' constantes for a gas are a=3.6 atmL^(2)mol^(-2),b=0.6Lmol^(-1) .If R=0.08LatmK^(-1)mol^(-1) and the Boyle's temperature (K) is T_(B) of this gas, then what is the value of (T_(B))/(15) ?

The van der Waals' constants of a gas are a=0.687dm^2mol^(-2)b=0.0226dm^3mol^(-1)

For a van der Waal's gas, determine Boyle Temperature (given a = 4.5 atm L^2 mol^(-2) , b = 0.9 L mol^(-1) and R = 0.082 L atm K^(-1) mol^(-1) ]

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

The van der Waal's constants a & b of CO_(2) are 3.64 L^(2) mol^(-2) bar & 0.04 L mol^(-1) respectively. The value of R is 0.083 bar dm^(3)mol^(-1)K^(-1) . If one mole of CO_(2) is confined to a volume of 0.15L at 300 K , then the pressure (in bar) eaxerted by the gas is :