When carbon is burned in air, it reacts with oxygen to form carbon dioxide. When 13.2 g of carbon were burned in the presence of 53.9 g of oxygen 18.7 g of oxygen remained unredacted. What mass of carbon dioxide was produced?

C + O2 - > CO2

Oxygen is the excess reactant (doesn't get used up in reaction, therefore mass of o2 is irrelevant) so use carbon (the limiting reactant) to calculate the mass of CO2

u should get 48.4g

grams of CO2 produced = 48.4 grams

Explanation:

Write the balance equation of the reaction. The chemical equation is represented below

C (s) + O2 (g) → CO2 (g)

The equation is already balanced. From the reaction carbon is the limiting reagent and it is use in the computation of mass for the product. Oxygen is in excess.

C (s) + O2 (g) → CO2 (g)

atomic mass of carbon = 12 g/mol

atomic mass of oxygen = 16 g/mol

Molar mass of carbon dioxide = 12 + 16 (2) = 12 + 32 = 44 grams

if 12 g of C produce 44 grams of CO2

13.2 grams of C will produce? grams of CO2

cross multiply

grams of CO2 produced = (13.2 * 44) / 12

grams of CO2 produced = 580.8/12

grams of CO2 produced = 48.4 grams