Vanderwaal's constant in litre atmosphere per mole for carbon dioxide are a = 3.6 and b = `4.28 xx 10^(-2)`. Calculate the critical temperature and critical volume of the gas. R = 0.0820 lit atm `K^(-1). Mol^(-1)`

Vanderwaal's constants for hydrogen chloride gas are a = 3.67 atm lit^(-2) and b = 40.8 ml mol^(-1) . Find the critical temperature and critical pressure of the gas.

Calculate the temperature of 4.0 mol of a gas occupying 5dm^3 at 3.32 bar. (R=0.083 ba r dm^3 K^-1 mol^-1) .

What is the density of N_2 gas at 227^@ C and 5.00atm. pressure? (R = 0.082 L atm K^(-1) mol^(-1))

Volume correction constant 'b' for argon gas is 3.22 xx 10^(-5) m^(3) per mol. Calculate the diameter of argon molecule.

Find the volume of 8g of oxygen gas at 27^@C and 1 atmosphere prressure. If the volume of each molecule is 3.4 xx 10^(-24)c c calculate the vacant space in the gas.

For the equilibrium A_((g)) + B_((g)) + C_((g)) , K_(p) = 0.82 atm at 27^(@)C . At the same temperature its K_(C) in mol li^(-1) is (R = 0.082 lit atm mol^(-1) K^(-1))

The volume to be excluded due to only two molecules of a gas in collision with a fixed point of impact is (0.09)/N_(A) litre (NA = Avogadro number). If the value of 'a' is 3.6 atm L^(2) mol^(-2) , then the value of Boyle's temperature is, 10^(x) K. What is the value of 'x' ? (R = 0.08 L atm K^(-1) m^(-1) )