Question

3) In the reaction below, how many grams of carbon dioxide are produced when iron III

oxide (Fe,O3) reacts completely with exactly 84 grams of carbon monoxide (CO)? Show
your work
Fe2O3 + 3C0> 2Fe + 3CO,
Molar masses:
CO = 289
CO2 = 449

Answer 1

132.03 g

Step-by-step explanation:

We are given;

• The equation for the reaction as;

Fe₂O₃ + 3CO → 2Fe + 3CO₂

• Molar masses of CO and CO₂ as 28.01 g/mol and 44.01 g/mol respectively
• Mass of CO as 84 grams

We are required to calculate the mass of CO₂ that will produced.

Step 1: Calculate the number of moles of CO

Moles = Mass ÷ Molar mass

Molar mass of CO = 28.01 g/mol

Therefore;

Moles of CO = 84 g ÷ 28.01 g/mol

= 2.9989 moles

= 3.0 moles

Step 2: Calculate the number of moles of CO₂

• From the reaction, 3 moles of CO reacts to produce 3 moles of CO₂

• Therefore; the mole ratio of CO to CO₂ is 1 : 1
• Hence; Moles of CO = Moles of CO₂

Moles of CO₂ = 3.0 Moles

But; mass = Moles × molar mass

Thus, mass of CO₂ = 3.0 moles × 44.01 g/mol

= 132.03 g

Hence, the mass of CO₂ produced from the reaction is 132.03 g