A 10 litre box contains `O_3` and `O_2` at equilibrium at 2000 K. `K_p=4xx10^(14)` atm for `2O_3(g)hArr 3O_2(g)`
Assume that `P_(O_2)gtgtP_(O_3)` and if total pressure is 8 atm, then partial pressure of `O_3` will be :

A 10 litre box contains O_3 and O_2 at equilibrium at 2000 k. K_p=4.17xx10^(14) "for" 2O_3 hArr 3O_2 Assume that P_(O_2) gt gt P_(O_3) and if total pressure is 7.33 atm. Then partial pressure of O_3 will be

A 10 litre box contains O_3 and O_2 at equilibrium at 2000 k. K_p=4.17xx10^(14) "for" 2O_3 hArr 3O_2 Assume that P_(O_2) gt gt P_(O_3) and if total pressure is 7.33 atm. Then partial pressure of O_3 will be

A(s) harr M(s) + 1/2O_2(g) K_p of the reaction is 4. Find the partial pressure of O_2 at equilibrium

The degree of dissociation of SO_(3) at equilibrium pressure is: K_(p) for 2SO_(3) (g)hArr2SO_(2)(g) + O_(2) (g)

A sample of pure NO_2 gas heated to 1000 K decomposes : 2NO_2(g) hArr 2NO(g)+O_(2)(g) The equilibrium constant K_P is 100 atm. Analysis shows that the partial pressure of O_2 is 0.25 atm. At equilibrium.The partial pressure of NO_2 at equilibrium is:

Density of O_3(g) at 2atm pressure and at 127°C is

Density of O_3(g) at 2atm pressure and at 127°C is

A vessel contains N_(2)O_(4) & NO_(2) in 2:3 molar ratio at 10 atm under equilibrium. Now, K_(P) for N_(2)O_(4) harr 2NO_(2) is