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_2O_4 and NO_2 at 1 atm is 3.62 g/L at 288 k and 1.84 g/L at 248 K. Calculate the entropy change during the reaction at 348 K.

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 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 and 373.5K is 2.0 g/L. Calculate K_(C) for the reaction N_(2)O_(2)(g) iff 2NO_(2)(g)

At 800 K in a sealed vessel for the equilibrium N_(2)(g) + O_(2) (g) hArr 2NO(g), the equilibrium concentrations of N_(2) (g), O_(2)(g) and NO(g) are respectively 0.36xx10^(-3) M, 4.41 xx 10^(-3) M and 1.4 xx 10^(-3) M. Calculate the value of K_(c) for the reaction NO(g) hArr 1//2 N_(2)(g) +1//2 O_(2) (g) at 800 K is :

For the equilibrium H_(2)O(l) iff H_(2)O(g) at 1 atm and 298 K