2. The decomposition of hydrogen sulfide occurs via the following reaction: 2H2S
ID: 706198 • Letter: 2
Question
2. The decomposition of hydrogen sulfide occurs via the following reaction: 2H2S(g)2H2(g) S2(9) At a temperature of 1065 C, this reaction does not go to completion. When 1.00 atm of H2S is put into a 5000-mL reaction vessel at a temperature of i065°C, only 24.0% of the HeS decomposes. The volume of the reaction vessel is held constant during the reaction a. How many moles of H2S are present before the reaction occurs? b. How many moles of H2S reacted? How many moles of H S are leftover? How many moles of H2 are produced? How many moles of S2 are produced? c. Calculate the partial pressure (in mmHg) of cach gascous species in the final reaction mixture. d. What is the total pressure (in mmHg) in the reaction vessel after the reaction?Explanation / Answer
2)
a) no of mol of H2S present(n) = PV/RT
= 1*0.5/(0.0821*1338.15)
= 0.00455 mol
b) no of mol of H2S reacted = 0.00455*24/100 = 0.001092 mol
no of mol of H2S left over = 0.00455 - 0.001092
= 0.003458 mol
no of mol of H2 produced = 0.001092*2
= 0.002184 mol
no of mol of S2 produced = 0.001092 mol
c) partial pressure of H2S leftover(Ph2s)= nRT/V
= 0.003458*0.0821*1338.15/0.5
= 0.76 atm
partial pressure of H2 (Ph2)= nRT/V
= 0.002184*0.0821*1338.15/0.5
= 0.48 atm
partial pressure of s2 (pS2) = 0.001092*0.0821*1338.15/0.5
= 0.24 atm
d) pTotal = pH2S+pH2+pS2
= 0.76+0.48+0.24
= 1.48 atm
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