" The equilibrium constant "Kp" for the reaction `NH_(4)HS_((s))to NH_(3(g))+H_(2)S_((g))` is

The equilibrium constant Kp for the reaction NH_(4)HS_((s)) Leftrightarrow NH_(3(g))+H_(2)S_((g)) is

The equilibrium constant for the reaction NH_(4)HS(s) Leftrightarrow NH_(3)(g)+H_(2)S(g) is correctly given by

A definite amount of solid NH_(4)HS is placed in a flask already containing ammonia gas at a certain temperature and 0.1 atm pressure. NH_(4)HS decompses to give NH_(3) and H_(2)S and at equilibrium total pressure in flask is 1.1 atm. If the equilibrium constant K_(P) for the reaction NH_(4)HS(s) iff NH_(3)(g)+H_(2)S(g) is represented as zxx10^(-1) then find the value of z.

The equilibrium constant for the reaction NH_(4)NO_(2)(s)hArr N_(2)(g)+2H_(2)O(g) , is given by

5 mole of NH_(4)HS(s) start to decompose at a particular temperature in a closed vessel. If pressure of NH_(3)(g) in the vessel is 2 atm, then K_(p) for the reaction, NH_(4)HS(s)hArrNH_(3)(g)+H_(2)S(g) , will be

The K_(p) of the reaction is NH_(4)HS_((s)) Leftrightarrow NH_(3(g))+H_(2)S_((g)) . If the total pressure at equilibrium is 30 atm.