Determine the volume of H₂S (at 375 K and 1.216 bar) needed to produce 55.0 g of S. Assume that there is excess SO₂ present.
2H₂S(g) + SO₂(g) → 3S(s) + 2H₂O(g)

Question

Quizplus · Accepted Answer

First, we need to calculate the moles of S, which is 55.0 g / 32.06 g/mol = 1.714 mol. From the balanced chemical equation, we can see that 2 moles of H₂S reacts to produce 3 moles of S. Therefore, the number of moles of H₂S required is: 1.714 mol S × (2 mol H₂S / 3 mol S) = 1.143 mol H₂S The ideal gas law can be used to calculate the volume of H₂S needed: PV = nRT V = nRT / P V = (1.143 mol) (0.08206 L·atm/mol·K) (375 K) / (1.216 atm) V = 29.3 L Therefore, the answer is B, 29.3 L.

Determine the Volume of H2S (At 375 K and 1

Determine the Volume of H₂S (At 375 K and 1