Final answer:
To find the volume of CO2, mass of Fe from Fe2O3, moles of Fe from CO, and molecules of CO required to produce Fe, we use stoichiometry based on the balanced chemical equation for the reaction between Fe2O3 and CO and apply molar relationships and conversions.
Step-by-step explanation:
To answer the student's questions, we need to consider the stoichiometry of the reaction between iron (III) oxide (Fe2O3) and carbon monoxide (CO), which produces iron (Fe) and carbon dioxide (CO2). The balanced chemical equation for this reaction is: Fe2O3 + 3CO → 2Fe + 3CO2.
1. The volume of carbon dioxide (CO2) produced when 2.90 moles of iron are produced can be calculated using the mole ratio from the balanced equation. For every 2 moles of Fe produced, 3 moles of CO2 are produced. Therefore, (2.90 moles Fe) x (3 moles CO2 / 2 moles Fe) = 4.35 moles CO2. We would then use the ideal gas law to convert moles of CO2 to volume at standard temperature and pressure (STP).
2. To determine the mass of iron that can be obtained from 3.80 g of Fe2O3, first calculate the moles of Fe2O3 using its molar mass. The mass of iron produced would then be calculated using the stoichiometry of the reaction and the molar mass of iron.
3. The moles of iron produced from 6.20 moles of CO is found by using the stoichiometric mole ratio from the balanced equation. Since 3 moles of CO produce 2 moles of Fe, (6.20 moles of CO) x (2 moles Fe / 3 moles CO) = 4.13 moles Fe.
4. To find out how many molecules of carbon monoxide (CO) are needed to react with excess Fe2O3 to produce 11.6 g of Fe, convert the mass of Fe to moles, use the stoichiometry of the reaction to find moles of CO, and then convert that to molecules.