When sulphur ( in the form of `S_(B))` is heated at temperature `T`, at equilibrium , the pressure of `S_(B)` falls by `30%` from `1.0 atm`, because `S_(B)(g)` in partially converted into `S_(2)(g)`. Find the value of `K_(P)` for this reaction.
When sulphur in the form of S_(8) is heated at 900 K , the initial pressure of 1 atm falls by 10% at equilibrium. This is because of conversion of some S_(8) to S_(2) . Find the value of equilibrium constant for this reaction.
When sulphur in the form of S_8 is heated at 900k the initial pressure of 1 atm falls by 29% at equilibrium . This is because of conversion of some S_8 "to" S_2 . Find the value of equilibrium constant for this reaction. S_8(g) hArr 4S_2(g)
When S in the form of S_(8) is heated at 900 K , the initial pressure of 1 atm falls by 29% at equilibrium. This is because of conversion of some S_(8) to S_(2) . Find the K_(p) for reaction.
When sulphur is heated at 900 K, S_(8) is converted to S_(2) . What will be the equilibrim constant for the reaction if initial pressure of 1 atm falls by 25% at equilibrium ?
For NH_4HS(s)hArrNH_3(g)+H_2S(g) , if K_p = 64 atm^2 , equilibrium pressure of mixture is
