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?

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

58750.08068 is the answer i think

what are the statements