When carbon is burned in air, it reacts with oxygen to form carbon dioxide. When 20.4 g of carbon were burned in the presence of 66.3 g of oxygen, 11.9 g of oxygen remained unreacted. What mass of carbon dioxide was produced?

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

C: 1 mole
O₂: 1 mole
CO₂: 1 mole

The molar mass of the compounds is:

C: 12 g/mole
O₂: 32 g/mole
CO₂: 44 g/mole

Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:

C: 1 mole ×12 g/mole= 12 grams
O₂: 1 mole ×32 g/mole= 32 grams
CO₂: 1 mole ×44 g/mole= 44 grams

Limiting reagent

The limiting reagent is one that is consumed first in its entirety, determining the amount of product in the reaction. When the limiting reagent is finished, the chemical reaction will stop.

Limiting reagent in this case

To determine the limiting reagent, you have to take in account that some oxygen remained unreacted. This is because it was present in excess. This means that the limiting reagent is carbon C.

Mass of CO₂ formed

Considering the limiting reagent, the following rule of three can be applied: if by reaction stoichiometry 12 grams of C form 44 grams of CO₂, 20.4 grams of C form how much mass of CO₂?

[tex]mass of CO_{2} =\frac{20.4 grams of Cx44 grams of CO_{2}}{12 grams of C}[/tex]

mass of CO₂= 74.8 grams

Then, 74.8 grams of CO₂ can be produced.

Learn more about the reaction stoichiometry:

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