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:
The molar mass of each compound is:
By reaction stoichiometry, the following amounts of mass of each compound participate in the reaction:
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?
[tex]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}}[/tex]
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.
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