Question

5)

What is the mass in grams of carbon dioxide, CO₂,
produced if 12.0 mol of iron are also produced?
Rxn A: 2Fe₂O3 + 3C → 4Fe + 3CO₂
Given:
Unknown:

Answer 1

To determine the mass of carbon dioxide produced in the reaction, we need to use the balanced chemical equation. The balanced equation for reaction A is:

2 Fe2O3 + 3 C -> 4 Fe + 3 CO2

The reaction tells us that for every 2 moles of Fe2O3, 3 moles of CO2 are produced. We are given the amount of Fe produced, which is 12 moles, so we can use that to determine the amount of Fe2O3 consumed and, therefore, the amount of CO2 produced.

First, let's calculate the amount of Fe2O3 consumed:

12 moles Fe / (4 moles Fe / 2 moles Fe2O3) = 6 moles Fe2O3

Next, we can use the ratio of Fe2O3 to CO2 from the balanced equation to calculate the amount of CO2 produced:

6 moles Fe2O3 * (3 moles CO2 / 2 moles Fe2O3) = 9 moles CO2

Finally, to convert moles to grams, we use the molar mass of CO2, which is 44.01 g/mol:

9 moles CO2 * 44.01 g/mol = 396.09 g CO2