question_answer

An amount of solid \[N{{H}_{4}}HS\] is placed in a flask already containing ammonia gas at a certain temperature and 1.0 atm pressure. Ammonium hydrogen sulphide decomposes to yield \[N{{H}_{3}}\] and \[{{H}_{2}}S\] gases in the flask. When the decomposition reaction reaches equilibrium, the total pressure in the flask rises to 2 atm. What will be the equilibrium constant for \[N{{H}_{4}}HS\] decomposition at this temperature?

Answer:

0.75