When carbon is burned in air, it reacts with oxygen to form carbon dioxide. When 16.8 gg of carbon were burned in the presence of 60.2 gg of oxygen, 15.4 gg of oxygen remained unreacted. What mass of carbon dioxide was produced?

61.6 g of CO₂ were produced

Explanation:

Let's think the combustion

C + O₂ → CO₂

First of all we determine the moles:

16.8 g. 1mol / 12 g = 1.4 moles

As the question states the oxygen is remained unreacted, the oxygen is the reactant in excess, so the limiting is the C.

1 mol of C produces 1 mol of CO₂, so 1.4 moles in the reactant will produce the same amount products.

We convert the moles to mass.

1.4 mol. 44 g / 1mol = 61.6 g