Question

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?

Answer 1

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

Answer 2

grams of CO2 produced = 48.4 grams

Step-by-step 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