What volume of water is produced when 38.5 g of ethanol reacts with oxygen at 500°C at 1.75 atm?
CH₃CH₂OH(g) + 3 O₂(g) → 2 CO₂(g) + 3 H₂O(g)

Question

What volume of water is produced when 38.5 g of ethanol reacts with oxygen at 500°C at 1.75 atm? CH₃CH₂OH(g)+ 3 O₂(g)→ 2 CO₂(g)+ 3 H₂O(g) A) 91.0 L B) 58.7 L C) 103 L D) 30.3 L E) 12.5 L

Quizplus · Accepted Answer

The balanced equation shows that 1 mole of ethanol produces 3 moles of water. The molar mass of ethanol is 46.07 g/mol, so 38.5 g of ethanol is 0.836 mol. Therefore, the reaction will produce 2.51 mol of water. At 500°C and 1.75 atm, the volume of 1 mol of gas is 30.3 L. Therefore, the volume of 2.51 mol of water is 2.51 mol x 30.3 L/mol = 76.0 L.

What Volume of Water Is Produced When 38