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Q.

When 5.1 g of solid NH₄HS is introduced into a two litre evacuated flask at 27 °C , 20% of the solid decomposes into gaseous ammonia and hydrogen sulphide. The K_P for the reaction at 27°C is x x 10^-2 .The value of x is ______.(Integer answer)

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answer is 6.

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Detailed Solution

Moles of ${NH}_{4} HS = \frac{5.1}{51} = 0.1 mole$
${NH}_{4 (s)} HS ⇌ {NH}_{3 (g)} + H_{2} s_{(g)}$
Initial moles 0.1 0 0
At time ‘t’ 0.1-0.02 0.02 0.02
$\begin{array}{l} p = \frac{nRT}{V} = \frac{0.02 \times 0.082 \times 300}{2} = 0.246 atm \\ K_{P} = [P_{{NH}_{3}}] [P_{H_{2} S}] \\ K_{p} = 0.246 \times 0.246 = 6.05 \times 10^{- 2} \\ \approx 6 \times 10^{- 2} \end{array}$

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