The combustion of ethanol (CH₃CH₂OH, 46.1 g/mol) results in the formation of water and carbon dioxide. How many grams of carbon dioxide are produced when 46.1 g of ethanol burns? A)88.0 g B)44.0 g C)176.0 g D)22.0 g E)11.0 g

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Quizplus · Accepted Answer

The balanced chemical equation for the combustion of ethanol (C2H5OH) is: C2H5OH + 3O2 → 2CO2 + 3H2O. From this equation, 1 mole of ethanol produces 2 moles of CO2. Since 46.1 g of ethanol is equivalent to 1 mole (given its molar mass is 46.1 g/mol), burning 46.1 g of ethanol will produce 2 moles of CO2. The molar mass of CO2 is 44.0 g/mol, so 2 moles of CO2 weigh 2 * 44.0 g = 88.0 g.

The Combustion of Ethanol (CH3CH2OH, 46

The Combustion of Ethanol (CH₃CH₂OH, 46