Consider the following reaction.How many moles of oxygen are required to produce 4.00 moles of water? Assume that there is excess C₃H₇SH present. C₃H₇SH(l)+ 6 O₂(g)→ 3 CO₂(g)+ SO₂(g)+ 4 H₂O(g) A) 2.67 moles O₂ B) 6.00 moles O₂ C) 4.00 moles O₂ D) 16.0 moles O₂ E) 1.00 moles O₂

Question

Quizplus · Accepted Answer

According to the balanced equation, it takes 6 moles of oxygen to produce 4 moles of water. Therefore, to produce 4.00 moles of water, we need (4/3) x 6 = 8 moles of oxygen. However, since the question assumes that there is excess oxygen present, we can safely say that we need 6.00 moles of oxygen to produce 4.00 moles of water.

Consider the Following Reaction