Determine the volume of H₂S (at 375 K and 1.20 atm)needed to produce 55.0 g of S.Assume that there is excess SO₂ present. 2 H₂S(g)+ SO₂(g)→ 3 S(s)+ 2 H₂O(g) A) 44.0 L B) 29.3 L C) 22.7 L D) 34.1 L E) 66.0 L

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To solve this problem, we need to use the ideal gas law to calculate the number of moles of H₂S needed to produce 55.0 g of S, and then use stoichiometry to convert that to the volume of H₂S at the given conditions. Step 1: Calculate the number of moles of S produced. 55.0 g S × (1 mol S/32.06 g S) = 1.718 mol S Step 2: Use stoichiometry to calculate the number of moles of H₂S needed. From the balanced equation, 2 H₂S(g) + SO₂(g) → 3 S(s) + 2 H₂O(g) we can see that 2 moles of H₂S produce 3 moles of S. Therefore, 1.718 mol S × (2 mol H₂S/3 mol S) = 1.145 mol H₂S Step 3: Use the ideal gas law to calculate the volume of H₂S at the given conditions. PV = nRT V = nRT/P V = (1.145 mol)(0.0821 L·atm/mol·K)(375 K)/(1.20 atm) V = 29.3 L Therefore, the answer is B.

Determine the Volume of H2S (At 375 K and 1

Determine the Volume of H₂S (At 375 K and 1