(a) State Dalton's law of partial pressure.
(b) The value of van der waals constant 'a' for `N_(2)` and `NH_(3)` are 1.37 and `4.30L^(2)*atm*mol^(-2)` respectively. Explain the difference in values.

(i) Any real gas behaves ideally at very low pressure and high temperature explain. (ii) The value of van der waals constant 'a' for N_(2) and NH_(3) are 1.37 and 4.30 L^(2)*atm*mol^(-2) respectively explain the difference in values.

The van dar waals constant 'a' for CO_(2) and CH_(4) gases are 3.6 and 2.3 L^(2)*atm*mol^(-2) . Which one of these two gases can easily be liquefied?

The values of van der Waal's constant a for the gases O_2,N_2,NH_3 and CH_4 is 1.360, 1.390, 4.170 and 2.253L^2 atm. mol^(-2) respectively. The gas which can most easily be liquefied is ?

The values of van der waals constants 'a' and 'b' for X, Y, and Z gases are 6,6,20 and 0.025, 0.15, 0.11, respectively. Which one has the highest critical temperature ?

If the orders of the values of van der waals constants a and b for three gases X, Y and Z are X lt Y lt Z and Z lt Y lt X respectively, then-

The inversion temperature Ti(K) of hydrogen is (Given van der Waal’s constant a and b are 0.244 atm L^2 mol^(-2) and 0.027 L mol^(-1) respectively.)

The vlaue of van der waals constant 'a' for nitrogen gas is 1.37L^(2)*atm*mol^(-2) , but that for ammonia gas is 4.30L^(2)*atm*mol^(-2) . What is the reason for this large difference ? Which one of these two gases would you expect to have higher critical temperature?

Given van der waals constant 'a' of NH_(3),H_(2),O_(2) and CO_(2) are respectively 4.17, 0.244, 1.36 and 3.59. which one of the following gases is most easily liquefied-

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

Establish the relation : Dalton's law of partial pressure: p=p_1+p_2+p_3+…..