Why `NO_2` dimerise to `N_2O_4` ?

NO_(2) dimerises to form N_(2)O_(4) . Why?

Why does NO_(2) dimerises.

1 mole of N_2O_4 is heated in a flask with a volume of 10 dm^3 . At equillibrium 1.708 mole of NO_2 and 0.146 mole of N_2O_4 were found at 134^@c calculate the equillibrium constant .

How is CH_3 CH_2 NH_2 prepared from C_2H_6 NO_2 ?

What is the oxidation number of chromium in K_2Cr_2O_7 and nitrogen in N_2H_4 ?

The standard heat of formation of NO_2(g) amd N_2O_4(g) are 8.0 2.0 kcal mol^-1 respectively. The heat of dimerization of NO_2 in kcal is:

One mole of N_2O_4 (g) at 300k is kept in a closed container under one atmospheric pressure. It is heated to 600 k when 20 % by mass of N_2O_4 (g) decomposes to NO_2(g) . The resultant pressure is :

Why does Nitrogen exist as N_2 white phosphorus as P_4 ?

The decomposition of N_2O_4 to NO_2 is carried out at 280 K in chloroform.When equiliberium has been established,0.2 mole of N_2O_4 and 2 xx 10^(-3) mole of NO_2 are present in a 2 litre solution. THE equiliberium constant for the reaction, N_2O_4 ⇌ 2NO_2 is :

The vapour density of undecomposed N_2O_4 is 46. When heated vapour density decreases to 24.5 due to its dissociation to NO_2 WHAT is the percent dissociation of N_2O_4 at the final stage ?