At `340 K` and `1` atm pressure, `N_(2)O_(4)` is `66%` into `NO_(2)`. What volume of `10 g N_(2)O_(4)` ocuupy under these conditions?

At 340 K and 1 atm pressure, N_(2)O_(4) is 66% into NO_(2) . What volume of 10 g N_(2)O_(4) occupy under these conditions?

N_(2)O_(4) is 60% dissociated into NO_(2) at 340K and 1 atm pressure. Find the volume of 10 g N_(2)O_(4) occupy under these condition.

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) ?

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 ?

N_2O_4 is 66% dissociated into NO_2 at 340 K and 1 atm pressure. Find the volume occupied by 10 g N_2O_4 , under these condition.

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?