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?

The combustion of ethanol is as follows;

C₂H₅OH + 3O₂ - - - > 2CO₂ + 3H₂O

stoichiometry of C₂H₅OH to CO₂ is 1:2

the mass of ethanol that was used - 46.1 g

Number of ethanol moles used up - 46.1 g / 46.1 g/mol = 1 mol

according to stoichiometry, when 1 mol of ethanol is used up, 2 mol of CO₂ is produced

Therefore mass of CO₂ produced - 2 mol x 44 g/mol = 88 g