`N_(2)O_(4)` dissociates into `NO_(2)`. If `%` dissociation of `N_(2)O_(4)` is `33.33 %`, calculate average molecular weight of gaseous mixture formed.

At 60^(@) and 1 atm, N_(2)O_(4) is 50% dissociated into NO_(2) then K_(p) is

At 60^(@) and 1 atm, N_(2)O_(4) is 50% dissociated into NO_(2) then K_(p) is

N_(2)O_(4) is 25% dissociated at 37^(@)C and 1 atm . Calculate K_(p)

Gaseous N_(2)O_(4) dissociates into gaseous NO_(2) according to the reaction : [N_(2)O_(4)(g)hArr2NO_(2)(g)] At 300 K and 1 atm pressure, the degree of dissociation of N_(2)O_(4) is 0.2. If one mole of N_(2)O_(4) gas is contained in a vessel, then the density of the equilibrium mixture is :

At 25^(@)C and 1 atm, N_(2)O_(4) dissociates the reaction N_(2)O_(4)(g) hArr 2NO_(2)(g) If it is 35% dissociated at given condition, find the volume of above mixture will difuse if 20 mL of pure O_(2) diffuse 10 minutes at same yemperature and pressure.

At 25^(@)C and 1 atm, N_(2)O_(4) dissociates the reaction N_(2)O_(4)(g) hArr 2NO_(2)(g) If it is 35% dissociated at given condition, find the volume of above mixture will difuse if 20 mL of pure O_(2) diffuse 10 minutes at same yemperature and pressure.

N_(2)O_(4) dissociates as N_(2)O_(4)hArr2NO_(2) . At 55^(@)C and one atmospehere, % decomposition of N_(2)O_(4) is 50.3% . At what P and same temperature, the equilibrium mixture will have the ratio of N_(2)O_(4):NO_(2) as 1:8 ?

A gaseous mixture contains 40% O_(2), 40% N_(2), 10% CO_(2), 10% CH_(4) by volume. Calculate the vapour density of the gaseous mixture.