When 189.6 g of ethylene (C2H4) burns in oxygen to give carbon dioxide and water, how many grams of CO2 are formed? C2H4 (g) + O2 (g) → CO2 (g) + H2O (g) (unbalanced)

596 g of CO₂ is the mass formed

Explanation:

Combustion reaction:

C₂H₄ (g) + 3O₂ (g) → 2CO₂ (g) + 2H₂O (g)

We determine moles of ethylene that has reacted:

189.6 g. 1mol / 28g = 6.77 moles

We assume the oxygen is in excess so the limiting reagent will be the ethylene.

1 mol of ethylene produce 2 moles of CO₂ then,

6.77 moles will produce the double of CO₂, 13.5 moles.

We convert the moles to mass: 13.5 mol. 44 g / 1mol = 596 g