Ethylene burns in oxygen to form carbon dioxide and water vapor:C2H4 + 3O2 ⟶ 2CO2 + 2H2OHow many liters of carbon dioxide can be formed if 49.75 L of ethylene at STP are consumed in this reaction?
Question
Ethylene burns in oxygen to form carbon dioxide and water vapor:C2H4 + 3O2 ⟶ 2CO2 + 2H2OHow many liters of carbon dioxide can be formed if 49.75 L of ethylene at STP are consumed in this reaction?
Solution
The reaction is balanced and shows that one molecule of ethylene (C2H4) produces two molecules of carbon dioxide (CO2).
In terms of moles, this means that one mole of ethylene produces two moles of carbon dioxide.
At Standard Temperature and Pressure (STP), one mole of any gas occupies 22.4 liters.
Therefore, the volume of ethylene (C2H4) given in the problem (49.75 L) corresponds to 49.75 L ÷ 22.4 L/mole = 2.22 moles of ethylene.
Since one mole of ethylene produces two moles of carbon dioxide, 2.22 moles of ethylene will produce 2.22 moles * 2 = 4.44 moles of carbon dioxide.
Finally, to convert this amount back to liters at STP, we use the fact that one mole of any gas occupies 22.4 liters. Therefore, 4.44 moles * 22.4 L/mole = 99.5 liters of carbon dioxide.
So, 49.75 liters of ethylene at STP will produce approximately 99.5 liters of carbon dioxide.
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