Ethanol is produced industrially by the acid catalyzed reaction of ethylene with water. The balanced equation for this reaction is:
C₂H₄(g) + H₂O(g) → C₂H₅OH(l)
If water is present in excess, how many grams of ethanol can be produced from 5.75 g of ethylene?

Question

Quizplus · Accepted Answer

The balanced equation for the reaction is C2H4(g) + H2O(g) → C2H5OH(l). The molar mass of ethylene (C2H4) is approximately 28.05 g/mol, and the molar mass of ethanol (C2H5OH) is approximately 46.07 g/mol. From 5.75 g of ethylene, the moles of ethylene are 5.75 g / 28.05 g/mol = 0.205 mol. Since the reaction is 1:1, this will produce 0.205 mol of ethanol. The mass of ethanol produced is 0.205 mol × 46.07 g/mol = 9.44 g.

Ethanol Is Produced Industrially by the Acid Catalyzed Reaction of Ethylene