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An amount of solid $\mathrm{NH}_4 \mathrm{HS}$ is placed in a flask already containing ammonia gas at a certain temperature and $0.50 \mathrm{~atm}$. Pressure. Ammonium hydrogen sulphide decomposes to yield $\mathrm{NH}_3$ and $\mathrm{H}_2 \mathrm{~S}$ gases in the flask. When the decomposition reaction reaches equilibrium, the total pressure in the flask rises to $0.84 \mathrm{~atm}$. The equilibrium constant for $\mathrm{NH}_4 \mathrm{HS}$ decomposition at this temperature is
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The correct answer is:
$0.11$
$0.11$
Total pressure $=0.5+2 \mathrm{x}=0.84$
i.e., $\mathrm{x}=0.17$
$\mathrm{~K}_{\mathrm{p}}=\mathrm{p}_{\mathrm{NH}_3} \cdot \mathrm{p}_{\mathrm{H}_2 \mathrm{~s}}$
$=(0.67) .(0.17)$
$\quad=0.1139$.
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