Oxygen and carbon monoxide react to form carbon dioxide as shown in the following reaction
O2 (g) + 2CO (g) - 2CO2 (g)
If a sample of 70.0 g of carbon monoxide was reacted with
32.0 g of oxygen, how many moles of carbon dioxide would be
produced?
moles

The number of moles of carbon dioxide that would be produced is 2 moles

Explanation:

The given reaction is presented as follows;

O₂ (g) + 2CO (g) → 2CO₂ (g)

The parameters given are;

The mass of the carbon monoxide, m₁ = 70.0 g

The mass of the oxygen, m₂ = 32.0 g

The molar mass of carbon monoxide = 28.01 g/mol

The molar mass of oxygen gas O₂ = 32.0 g/mol

The number of moles, n = (The mass)/(The Molar Mass)

The number of moles of carbon monoxide in the reaction = 70.0 g/(28.01 g/mol) = 2.49910746 moles ≈ 2.5 moles

The number of moles of oxygen in the reaction = 32.0 g/(32.0 g/mol) = 1 moles

Therefore, from the chemical reaction, we have;

One mole of O₂ reacts with two moles of  CO  to produce two moles of CO₂ (g)

1 mole of oxygen produces 2 moles of carbon dioxide

Therefore, given that the number of moles of oxygen in the reaction is 1  mole, we have that the number of moles of carbon dioxide that would be produced = 2 moles.

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