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?

For the dissociation reaction N_(2)O_(4)(g)hArr2NO_(2)(g), the equilibrium constant K_(P) is 0.120 atm at 298 K and total pressure of system is 2 atm. Calculate the degree of dissociation of N_(2)O_(4) .

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.

For the dissociation reaction N_(2)OhArr2NO_(2)(g), the equilibrium constant K_(P) is 0.120 atm at 298 K and total pressure of system is 2 atm. Calculate the degree of dissociation of N_(2)O_(4) .

The equilibrium constant K_(p) for the following reaction is 4.5 N_(2)O_(4)(g)hArr2NO_(2)(g) What would be the average molar mass ("in"g//mol) of an equilibrium mixture of N_(2)O_(4) and NO_(2) formed by the dissociation of pure N_(2)O_(4) at a total pressure of 2 atm ?

The equilibrium constant K_(p) for the following reaction is 4.5 N_(2)O_(4)(g)hArr2NO_(2)(g) What would be the average molar mass ("in"g//mol) of an equilibriumm mixture of N_(2)O)(4) and NO_(2) formed by the dissociation of pure N_(2)O_(4) at a jtotal pressure of 2 atm ?

The equilibrium constant K_(p) for the following reaction is 4.5 N_(2)O_(4)(g)hArr2NO_(2)(g) What would be the average molar mass ("in"g//mol) of an equilibriumm mixture of N_(2)O)(4) and NO_(2) formed by the dissociation of pure N_(2)O_(4) at a jtotal pressure of 2 atm ?

The equilibrium constant K_(P) for the reaction N_(2)O_(4)(g) hArr 2NO_(2)(g) is 4.5 atm . What would be the average molar mass (in g//mol ) of an equilibrium mixture at a total pressure of 2 atm of N_(2)O_(4) and NO_(2) formed by the dissociation of pure N_(2)O_(4) ?