When 3.06g of solid `NH_4HS` is introduced into a 21 evacuated flask at `27^(@)`C, 30% of the solid decomposes into gaseous ammonia and hydrogen sulphide.
what would happen to the equilibrium when more solid `NH_4HS` is introduced into the flask?

Explanation

`logK=(/_\G^0)/(2.303RT)=(2xx10^3)/(2.303xx8.314xx500)=-0.209`
`:.K=0.618`
For equilibrium, `2A+B Therefore, for equilibrium,
`A+1/2B