SATHEE: Chemical and Ionic Equilibrium

Chemical and Ionic Equilibrium - Result Question 100

####44. When $3.06 g$ of solid $N H_{4} S H$ is introduced into a two litre evacuated flask at $27^{\circ} C, 30$ of the solid decomposes into gaseous ammonia and hydrogen sulphide.

(i) Calculate $K_{c}$ and $K_{p}$ for the reaction at $27^{\circ} C$ .

(ii) What would happen to the equilibrium when more solid $N H_{4} S H$ is introduced into the flask?

$(1999, 7 M)$

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Solution:

(i) Mole of solid $N H_{4} H S$ taken initially $= \frac{3.06}{51} = 0.06$

$\begin{aligned} At equilibrium N H_{4} H S (s) ⇌ \underset{0.018}{N H_{3} (g) +} H_{2} S (g) & K_{c} = {(\frac{0.018}{2})}^{2} = 8.1 \times 10^{- 5} & p (N H_{3}) = \frac{0.018 \times 0.082 \times 300}{2} = 0.22 a t m & K_{p} = (0.22)^{2} = 4.84 \times 10^{- 2} \end{aligned}$

(ii) Addition of solid $N H_{4} H S$ will have no effect on equilibrium.

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Chemical and Ionic Equilibrium - Result Question 100

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