When 233.1 g of ethylene (C₂H₄)burns in oxygen to give carbon dioxide and water,how many grams of CO₂ are formed? A)731.4 g B)365.7 g C)182.9 g D)8.31 g E)299.4 g

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The balanced chemical equation for the combustion of ethylene (C2H4) is: C2H4 + 3O2 -> 2CO2 + 2H2O. The molar mass of ethylene (C2H4) is approximately 28.05 g/mol, and the molar mass of CO2 is approximately 44.01 g/mol. Given 233.1 g of ethylene, we first find the moles of ethylene: 233.1 g / 28.05 g/mol = 8.31 moles of C2H4. From the balanced equation, 1 mole of C2H4 produces 2 moles of CO2, so 8.31 moles of C2H4 will produce 8.31 * 2 = 16.62 moles of CO2. The mass of CO2 produced is 16.62 moles * 44.01 g/mol = 731.4 g.

When 2331 G of Ethylene (C2H4)burns in Oxygen to Give Carbon

When 2331 G of Ethylene (C₂H₄)burns in Oxygen to Give Carbon