Density of equilibrium mixture of `N_(2)O_(4)` and `NO_(2)` at `1 atm` and `384 K` is `1.84 g dm^(-3)`. Calculate the equilibrium constant of the reaction.
`N_(2)O_(4)hArr2NO_(2)`

The density of an equilibrium mixture of N_(2)O_(4) and NO_(2) at 1 atm and 373.5K is 2.0 g/L. Calculate K_(C) for the reaction N_(2)O_(2)(g) iff 2NO_(2)(g)

The density of an equilibrium mixture of N_(2)O_(4) and NO_(2) at 1 atm is 3.62 g L^(-1) at 288 K and 1.84 g L^(-1) at 348 K . Calculate the entropy change during the reaction at 348 K .

The equilibrium constant for the reaction NH_(4)NO_(2)(s)hArr N_(2)(g)+2H_(2)O(g) , is given by

The equilibrium constant for the given reaction is 100. N_(2)(g)+2O_(2)(g) hArr 2NO_(2)(g) What is the equilibrium constant for the reaction ? NO_(2)(g) hArr 1//2 N_(2)(g) +O_(2)(g)

Vapour density of the equilibrium mixture of NO_(2) and N_(2)O_(4) is found to be 40 for the equilibrium N_(2)O_(4) hArr 2NO_(2) Calculate