At `27^(@)C` and 1 atm pressure , `N_(2)O_(4)` is `20%` dissociation into `NO_(2)`. What is the density of equilibrium mixture of `N_(2)O_(4)` and `NO_(2)` at `27^(@)C` and 1 atm ?

At 27^(@)C and 1 atm pressure , N_(2)O_(4) is 20% dissociation into NO_(@) .What is the density of equilibrium mixture of N_(2)O_(4) and NO_(2) at 27^(@)C and 1 atm?

At 27^(@)C and 1 atm pressure , N_(2)O_(4) is 20% dissociation into NO_(@) .What is the density of equilibrium mixture of N_(2)O_(4) and NO_(2) at 27^(@)C and 1 atm?

At 27^(@)C and 1 atm pressure , N_(2)O_(4) is 20% dissociation into NO_(@) .What is the density of equilibrium mixture of N_(2)O_(4) and NO_(2) at 27^(@)C and 1 atm?

At 27^@C and 1 atmosphere pressure N_2O_4 is 20% dissociated into NO_2 find K_P

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

At 77^(@)C and one atmospheric pressure , N_(2)O_(4) is 70% dissociated into NO_(2) What will be the volume occupied by the mixture under these conditions if we start with 10 g of N_(2)O_(4) ?

A given sample of N_(2)O_(4) in a closed vessel shows 20% dissociation in NO_(2) at 27^(@)C and 760 "torr" . The sample is now heated upto 127^(@)C and the analysis of mixture shows 60% dissociation at 127^(@)C . The density of the equilibrium mixture (in g//litre ) at 27^(@)C is :

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