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:

At 1000 K , a sample of pure NO_(2) gases decomposes as : 2NO_(2)(g)hArr2NO(g)+O_(2)(g) The equilibrium constant K_(P) is 156.25 atm .Analysis showns that the partial pressure of O_(2) is 0.25 atm at equilibrium .The parital pressure o f NO_(2) at equilibrium is :

At 1000 K , a sample of pure NO_(2) gases decomposes as : 2NO_(2)(g)hArr2NO(g)+O_(2)(g) The equilibrium constant K_(P) is 156.25 atm .Analysis showns that the partial pressure of O_(2) is 0.25 atm at equilibrium .The parital pressure o f NO_(2) at equilibrium is :

At 1000 K , a sample of pure NO_(2) gases decomposes as : 2NO_(2)(g)hArr2NO(g)+O_(2)(g) The equilibrium constant K_(P) is 156.25 atm .Analysis showns that the partial pressure of O_(2) is 0.25 atm at equilibrium .The parital pressure o f NO_(2) at equilibrium is :

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

C(s)+CO_(2)(g) iff 2CO(g) . At equilibrium, 25% of the CO_(2) got converted into CO. If the equilibrium pressure is 12 atm, the partial pressure of CO_(2) at equilibrium is

At a particular temperature, the value of K_(p) is 100 for the reaction, 2NO(g)hArrN_(2)(g)+O_(2)(g) occurring in a closed container. If the iniital pressure of NO(g) be 25 atm then calculate the partial pressures of NO, N_(2) and O_(2) at equilibrium.