When \( 3.06 \mathrm{~g} \) of solid \( \mathrm{NH}_{4} \mathrm{HS} \) is introduced into a two ...

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When \( 3.06 \mathrm{~g} \) of solid \( \mathrm{NH}_{4} \mathrm{HS} \) is introduced into a two litre evacuated flask at \( 27 \mathrm{C}, 30 \% \) of the solid decomposes into gaseous ammonia and hydrogen sulphide.
(i) Calculate \( \mathrm{K}_{\mathrm{C}} \& \mathrm{~K}_{\mathrm{p}} \) for the reaction at \( 27 \mathrm{C} \).
(ii) What would happen to the equilibrium when more solid \( \mathrm{NH}_{4} \mathrm{HS} \) is introduced into the flask?
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