Chemistry

Problem

When

3.06 \text{ g}

of solid

\text{NH}_4\text{HS}

is introduced into a two-litre evacuated flask at

27^\circ\text{C}

30\%

of the solid decomposes into gaseous ammonia and hydrogen sulphide. (IIT 1999) (i) Calculate

K_C

and

K_P

for the reaction at

27^\circ\text{C}

. (ii) What would happen to the equilibrium when more solid

\text{NH}_4\text{HS}

is introduced into the flask ?