When `3.06 g` of 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)HS` is introduced into the flask?

Explanation

`(i) 8.1 xx 10^(-5) ` mole/L , `0.049 atm^(-2)`, (ii) no effect