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

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the practice of taking someone else's work or ideas and passing them off as one's own.

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answers: to make sure that all of the broken pieces of tablet were added to the water, to allow for fair comparison of all three trials, with different particle sizes to avoid experimental error