The combustion of ethanol (CH₃CH₂OH, 46.7 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?

Question

Quizplus · Accepted Answer

The balanced chemical equation for the combustion of ethanol (C2H5OH) is: C2H5OH + 3O2 → 2CO2 + 3H2O. From the equation, 1 mole of ethanol produces 2 moles of CO2. The molar mass of ethanol is 46.07 g/mol, so 46.1 g of ethanol is approximately 1 mole. Therefore, 1 mole of ethanol produces 2 moles of CO2, which is 44.01 g/mol * 2 = 88.02 g of CO2. The closest answer is 88.1 g.

The Combustion of Ethanol (CH3CH2OH, 46

The Combustion of Ethanol (CH₃CH₂OH, 46