When carbon is burned in air, it reacts with oxygen to form carbon dioxide. When 24.0 g of carbon were burned in the presence of 82.9 g of oxygen, 18.9 g of oxygen remained unreacted. What mass of carbon dioxide was produced?

88 g of CO₂ were produced by this reaction

Explanation:

We determine the combustion:

C(s) + O₂(g) → CO₂(g)

If the problem states, that oxygen has remained after the reaction is complete, the O₂ is the excess reactant and the limiting.

We convert mass to moles → 24 g . 1mol / 12g = 2 moles

As ratio is 1:1, 2 moles of C must produce 2 moles of CO₂

We convert the moles to mass:

2mol . 44g/ 1mol = 88 g

each  column  of the  table  is called a group. elements in a group share similar properties. groups are  read  from  top  to  bottom. metal. metalloid. nonmetal. solid. liquid. gas. fe. hg. o.  2. 3. 4. 5. 6. 7. 8. 9.  2. beryllium. 9.012. 4.  sodium. 22.990.  11. 3.  magnesium. 24.305.  12.  potassium. 39.098.  19. 4.  calcium. 40.078.  20. i guess  i