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An amount of solid NH(4)HS is placed in...

An amount of solid `NH_(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 `NH_(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 `NH_4HS` decomposition at this temperature?

Text Solution

Verified by Experts

The correct Answer is:
0.75
`underset("initial At. Eqn")(NH_(4)HS(s)) Then, `1.0 + x + x=2x+1.0=2.0` (given)
`rArr x=0.5` atm
`P_(NH-(3)) =1.0 + 1.5 1.5 atm, p-(H_(2)S) = 0.5 atm^(2)`
`0.75 atm^(2)`
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