Answer:
We need 29.2 L of H2S
Explanation:
Step 1: Data given
Volume of H2S = TO BE DETERMINED
Temperature = 375 K
Pressure = 1.20 atm
Mass of S = 55.0 grams
Molar mass of S = 32.065 g/mol
Step 2: The balanced equation:
2H2S(g) + SO2(g) ⇒ 3 S(s) + 2 H2O(g)
Step 3: Calculate moles of S
Moles of S = Mass S / molar mass of S
Moles of S = 55.0 grams / 32.065 g/mol
Moles of S = 1.715 moles
Step 4: Calculate moles of H2S
For 2 moles of H2S we need 1 mol of SO2 to produce 3 moles of S and 2 moles of H2O
For 1.715 moles S we need, (2/3)*1.715 = 1.14 moles of H2S
Step 5: Calculate volume of H2S
p*V=n*R*T
⇒ p = the pressure of H2S = 1.20 atm
⇒ V = The volume of H2S = TO BE DETERMINED
⇒ n = the moles of H2S = 1.14 moles H2S
⇒ R = the gas constant = 0.08206 L*atm/K*mol
⇒ T = The temperature = 375 K
V= (n*R*T)/P
V = (1.14*0.08206*375)/1.20
V = 29.2 L
We need 29.2 L of H2S
