When 3*06of solid NH_(4)HS is introduced into a two - litre evacuated flask at 27^(@C,30% of the solid decomposes into gaseous ammonia and hydrogen sulphide. (i) Calculate K_(c) and K _(p) for the reaction at 27^(@)C. (ii) What would happen to the equilibrium when more solid NH_(4)HSis introduced into the flask ?

When 3*06of solid NH_(4)HS is introduced into a two - litre evacuated

1.	When 3*06of solid NH_(4)HS is introduced into a two - litre evacuated flask at 27^(@C,30% of the solid decomposes into gaseous ammonia and hydrogen sulphide. (i) Calculate K_(c) and K _(p) for the reaction at 27^(@)C. (ii) What would happen to the equilibrium when more solid NH_(4)HSis introduced into the flask ?
Answer» Solution :` {:((i),NH_(4)HS(s),HARR,NH_(3)(s),+,H_(2)S(g)), ("Intial amount",306 g,,,,), (,=306//51 "mole",,,,),(,=006 "mole",,,,):}` `{:("At eqm.",006-30/100xx006,0018 "mole",0018"mole"), (,=006-0018,,), (,=0042 "mole",,):}` ` {:("Eqm.conc",1,0018//2,0018//2),(,("being solid"),=0009,=0009"mol"L^(-1)):}` ` K_(c) = ([NH_(3)][H_(2)S])/([NH_(4)HS])=(0009 xx 0009)/1 = 8*1 xx10^(-5)"" ( [NH_(4)HS(s)] = 1 ) ` ` K_(p)= K_(c) (RT)^(Delta n_(g)) = 2 -0 =2` (II)As`K_(c) = [NH_(3)][H_(2)S] `and does not depend upon the amount of `NH_(4)HS`(s) . hence , therewill be no effect on equilibrium when more solid `NH_(4)HS ` is added.