Answer to Question #350674 in Chemistry for Cow

Question

5. How many moles of CO, (carbon dioxide) are produced when 5.5 moles of Oz

(oxygen) is used in the reaction below?

26gH18 + 2502 - 16CO2+ 18H20

B. How many grams of oxygen is that?

Answer 1

Solution:

Balanced chemical equation:

2C₈H₁₈ + 25O₂ → 16CO₂ + 18H₂O

According to stoichiometry:

25 mol of O₂ produce 16 mol of CO₂

Thus, 5.5 mol of O₂ produce:

(5.5 mol O₂) × (16 mol CO₂ / 25 mol O₂) = 3.52 mol CO₂

3.52 moles of CO₂ (carbon dioxide) are produced

The molar mass of O₂ is 32 g/mol

Therefore,

Mass of O₂ = (5.5 mol O₂) × (32 g O₂ / 1 mol O₂) = 176 g O₂

176 grams of oxygen is that

Answer:

3.52 moles of CO₂ (carbon dioxide) are produced;

176 grams of oxygen is that.