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When 3.06 g of solid NH(4)HS is introduc...

When `3.06 g` of solid `NH_(4)HS` is introduced into a two-litre evacuated flask at `27^(@)C, 30%` of the solid decomposes into gaseous ammonia and hydrogen sulphide. (i) Calculate `K_(c )` and `K_(p)` for the reaction at `27^(@)C`. (ii) What would happen to the equilibrium when more solid `NH_(4)HS` is introduced into the flask?

A

`8.1 xx10^(-4) and 3.9 xx10^(-2)`

B

`0.8xx10^(-5) and 4.9xx10^(-5)`

C

`9.1xx10^(-3)and 4.9xx10^(-3)`

D

`8.1xx10^(-5) and 4.9xx10^(-2)`

Text Solution

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The correct Answer is:
D
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