Question

What is the mass in grams of oxygen gas that is required to produce 32.1 grams of maleic acid anhydride?

Answer 1

Considering the reaction stoichiometry, the mass of oxygen gas that is required to produce 32.1 grams of maleic acid anhydride is 47.17 grams.

The balanced reaction is:

2 C₆H₆(l) + 9 O₂(g)→ 2 C₄H₂O₃(s) + 4 CO₂(g) + 4 H₂O(g)

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

• C₆H₆: 2 moles
• O₂: 9  moles
• C₄H₂O₃: 2 moles
• CO₂: 4 moles
• H₂O: 4 moles

The molar mass of each compound is:

• C₆H₆: 78 g/mole
• O₂: 32 g/mole
• C₄H₂O₃: 98 g/mole
• CO₂: 44 g/mole
• H₂O: 18 g/mole

By reaction stoichiometry, the following amounts of mass of each compound participate in the reaction:

• C₆H₆: 2 moles× 78 g/mole= 156 grams
• O₂: 9 moles× 32 g/mole= 288 grams
• C₄H₂O₃: 2 moles× 98 g/mole= 196 grams
• CO₂: 4 moles× 44 g/mole= 176 grams
• H₂O: 4 moles× 18 g/mole= 72 grams

Then you can apply the following rule of three: If by stoichiometries 196 grams of C₄H₂O₃ are produced by 288 grams of O₂, 32.1 grams of C₄H₂O₃ are produced from how much mass of O₂?

$mass of O_{2} =\frac{32.1 grams of C_{4} H_{2} O_{3} x288 grams of O_{2}}{196grams of C_{4} H_{2} O_{3}}$

mass of O₂= 47.17 grams

Finally, the mass of oxygen gas that is required to produce 32.1 grams of maleic acid anhydride is 47.17 grams.  

Learn more:

• brainly.com/question/16487206?referrer=searchResults
• brainly.com/question/14446695?referrer=searchResults
• brainly.com/question/11564309?referrer=searchResults