The equilibrium constant `(K_P)` of the reactions `N_2O_4hArr 2NO_2` was found to be 636 mm at ` 49.7""^(@) C ` . Calculate the percentage dissociation of `N_2O_4` when the pressure of the gas mixture is 182 mm.

The equilibrium constant K_(p) for the reaction N_(2)O_(4)(g)hArr2NO_(2)(g) at 497^(@)C is found to be 636 mm Hg . If the pressure of the gas mixture is 182 mm , calculate the presentage dissociation of N_(2)O_(4) . At what pressure will it be dissociated?

The K_P for the reaction N_2O_4 hArr 2NO_2 is 640 mm at 775 K.The percentage dissociation of N_2O_4 at equilibrium pressure of 160 mm is :

At the equilibrium of the reaction , N_(2)O_(4)(g)rArr2NO_(2)(g) , the observed molar mass of N_(2)O_(4) is 77.70 g . The percentage dissociation of N_(2)O_(4) is :-

The equllibrium constant K_c for the reaction. N_2O_4 hArr2NO_2(g) "is" 4.63xx10^(-3) "at" 25^@C What is the value of K_p at this temperature.

The vapour density of N_(2)O_(4) at a certain temperature is 30 . Calculate the percentage dissociation of N_(2)O_(4) this temperature.

Write the equilibrium constant expressions for the following reactions. N_2 O_4 g hArr 2NO_2 (g)

K_p for the reaction N_2O_4 (g) hArr 2NO_2(g) is 0.66 at 46^@C . Calculate the part per cent dissociation of N_2O_4 at 46^@C and a total pressure of 0.5 atm. Also calculate the partial pressure of N_2O_4 and NO_2 at equilibrium .

For the reaction N_2O_4 hArr 2NO_2(g) , if percentage dissociation of N_2O_4 are 20%, 45%, 65%, 80% then the sequence of observed vapour densities wil be :

Write the equilibrium constant expressions for the following reactions. N_2(g) +O_2(g)hArr 2NO(g)

If in the reaction, N_(2)O_(4)(g)hArr2NO_(2)(g), alpha is the degree of dissociation of N_(2)O_(4) , then the number of moles at equilibrium will be