Vanderwaal's constant 'a' has the dimensions of (A) `mol L^(-1)` (B) `atm L^2 mol^(-2)` (C) `litre``mol^(-1)` (D) `atm L mol^(-2)`

The values of the van der Waals' constant a for some gases are given below. H_2 = 0.245 " atm " L^2 mol^(-2) O_2 = 1.360 " atm " L^2 mol^(-2) CO_2 = 3.590 " atm " L^2 mol^(-2) NH_3 = 4.170 " atm " L^2 mol^(-2) Arrange these gases in the decreasing order of their liquefaction tendencies.

What is the value if R when its units are L atm K^(-1) mol^(-1) ?

Calculate the value of R in : (i) SI units , (II) Cal "degree"^(-1) "mol"^(-1) , (iii) Litre atm K^(-1) "mol"^(-1)

Identify the reaction order from each of the following rate constants (i) k= 3 xx 10^(-5) s^(-) (ii) k=9 xx 10^(-4) mol ^(-) "litre "s^(-) (iii) k= 6 xx 10^(-2) litre mol ^(-) s^(-) (iv) k= 2.3 xx 10^(-5) L mol ^(-1) s^(-1) (v) k= 3 xx 10^(-3) mol L^(-1) s^(-1)

The units of molarity is mol.L

What is the compressibility factor (Z) for 0.02 mole of a van der Waals's gas at pressure of 0.1 atm. Assume the size of gas molecules is negligible. Given : RT=20 L atm mol^(-1) and a=1000 atm L^(2) mol^(-2)

Calculate the pressure exerted by one mole of methane in a 450 mL container at 25^@C using van der Waals' equation. What pressure will be predicted by ideal gas equation ? (Given : a = 2.253 " atm " L^2 mol^(-2), b = 0.0428 L mol^(-2), R =0.0821 L " atm " K^(-1) mol^(_1))

Rate constant k = 1.2 xx 10^(3) mol^(-1) L s^(-1) and E_(a) = 2.0 xx 10^(2) kJ mol^(-1) . When T rarr oo :