Determine the theoretical yield of H₂S (in moles) if 4.0 mol Al₂S₃ and 4.0 mol H₂O are reacted according to the following balanced reaction. A possibly useful molar mass is Al₂S₃= 150.17 g mol^-1. Al₂S₃(s) + 6H₂O(l) → 2Al(OH)₃(s) + 3H₂S(g) A) 12 mol H₂S B) 4.0 mol H₂S C) 18 mol H₂S D) 6.0 mol H₂S E) 2.0 mol H₂S

Question

Quizplus · Accepted Answer

The reaction requires 6 moles of H₂O for every mole of Al₂S₃. With 4.0 mol Al₂S₃, you would need 24 mol H₂O, but only 4.0 mol H₂O is available, making H₂O the limiting reactant. Thus, 4.0 mol H₂O can produce (4.0 mol H₂O / 6 mol H₂O) * 3 mol H₂S = 2.0 mol H₂S.

Determine the Theoretical Yield of H2S (In Moles) If 4

Determine the Theoretical Yield of H₂S (In Moles) If 4