Consider the chemical equation, 2H₂+O₂ → 2H₂O (Molar masses: H₂ = 2.016 g; O₂ = 32 g; H₂O = 18.016 g). If the percent yield of this reaction is estimated to be only 90%, calculate the amount of water that can be produced from 90.00 g oxygen.

Question

Quizplus · Accepted Answer

First, calculate the moles of O₂: 90.00 g / 32 g/mol = 2.8125 mol. According to the balanced equation, 1 mol O₂ produces 2 mol H₂O, so 2.8125 mol O₂ produces 5.625 mol H₂O. Theoretical mass of H₂O = 5.625 mol × 18.016 g/mol = 101.325 g. Considering 90% yield: 101.325 g × 0.9 = 91.1925 g, which rounds to 91.2 g.

Consider the Chemical Equation, 2H2+O2 → 2H2O (Molar Masses: H2

Consider the Chemical Equation, 2H₂+O₂ → 2H₂O (Molar Masses: H₂