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)`

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)

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 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 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 N_(2)(g)+O_(2)(g) hArr 2NO(g) at temperature T is 4xx10^(-4) . The value of K_(c) for the reaction NO(g) hArr 1/2 N_(2)(g)+1/2 O_(2)(g) at the same temperature is

The equilibrium constant for the reaction N_(2)(g)+O_(2)(g) hArr 2NO(g) at temperature T is 4xx10^(-4) . The value of K_(c) for the reaction NO(g) hArr 1/2 N_(2)(g)+1/2 O_(2)(g) at the same temperature is

The equilibrium constant for the reaction N_(2)(g)+O_(2)(g) hArr 2NO(g) at temperature T is 4xx10^(-4) . The value of K_(c) for the reaction NO(g) hArr 1/2 N_(2)(g)+1/2 O_(2)(g) at the same temperature is

The equilibrium constant for the reaction N_(2)(g)+O_(2)(g) hArr 2NO(g) at temperature T is 4xx10^(-4) . The value of K_(c) for the reaction NO(g) hArr 1/2 N_(2)(g)+1/2 O_(2)(g) at the same temperature is

The equilibrium constant for the reaction N_(2)(g)+O_(2)(g) hArr 2NO(g) at temperature T is 4xx10^(-4) . The value of K_(c) for the reaction NO(g) hArr 1/2 N_(2)(g)+1/2 O_(2)(g) at the same temperature is