When 5.1 g of solid NH_4HS is introduced into a two litre evacuated flask at 27°C, 20% of the solid decomposes into gaseous ammonia and hydrogen…

Question

When 5.1 g of solid NH_4HS 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×10^(-2). The value of x is (Integer answer) [Given 1R=0.082 L atm K^(-1) mol^(-1)

MARKS Content Team · Accepted Answer

Correct answer: 6. Moles of NH_4HS initially taken =(5.1 g)/(51 g/mol)=0.1 mol volume of vessel =2 L NH_4HS_((s))⇌NH_(3( g))+H_2S_((g)) t=0 0.1 mol t=∞ 0.1(1-0.2) 0.1×0.2 0.1×0.2 Partial pressure of each gaseous component P=nRT/V=(0.1×0.2×0.082×300)/2 =0.246 atm ⇒k_P=P_NH3×P_(H2 S)=(0.246)^2=0.060516 =6.05×10^(-2) ⇒6

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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 Kp for the reaction at 27°C is x×10-2. The value of x is (Integer answer)[Given 1R=0.082 L atm K-1 mol-1

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