5.1g NH_4 SH is introduced in 3.0L evacuated flask at 327°C ,30 \% of the solid NH_4 SH decomposed to NH_3 and H_2as gases. The K_p of the reaction at 327°C is (R=0.082L mol^-1, molar mass of S=32g m…

Question

5.1g NH_4 SH is introduced in 3.0L evacuated flask at 327°C ,30 \% of the solid NH_4 SH decomposed to NH_3 and H_2as gases. The K_p of the reaction at 327°C is (R=0.082L mol^-1, molar mass of S=32g mol^-1, molar massof (N=14g mol^-1)

Accepted Answer

Correct answer: D. (d) Concerned reaction: NH_4 SH ⟶ NH_3 (g )+H_2S (g ) Initial moles = 5.151=0.1 mol Moles at equilibrium NH_4 SH0.1 (1-0.3 ) ⟶ NH_3 (g )0.1 0.3+H_2S (g )0.1 0.3 ∴K_c= ( NH_3 ) (H_2S )= ( 0.033 )^2=10^-4 K_p=K_c ( RT )^ n_g =10^-4 (0.082 600 )^2=0.242 atm^2

$5.1 g NH_{4} SH is introduced in 3.0 L evacuated flask at 327° C, 30 % of the solid NH_{4} SH decomposed to NH_{3} and H_{2} as gases. The K_{p} of the reaction at 327° C is (R = 0.082 L mol^{- 1}, molar mass of S = 32 g mol^{- 1}, molar massof (N = 14 g mol^{- 1})$

Solution

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