Final answer:
Determining the truthfulness of the statement requires stoichiometric calculations based on the chemical reaction between iron(III) oxide and carbon. However, the question is missing crucial information to calculate the exact mass of iron produced, making it impossible to confidently label the statement as true or false.
Step-by-step explanation:
The question asks if combining 0.339 mol Fe2O3 with excess carbon produced 11.7 g Fe is true or false. To answer this, we can use stoichiometric calculations. The reaction between Fe2O3 and carbon is a reduction reaction, where iron(III) oxide (Fe2O3) is reduced to elemental iron (Fe):
Fe2O3 (s) + 3C (s) → 2Fe (s) + 3CO (g)
According to the stoichiometry of the reaction, 1 mole of Fe2O3 produces 2 moles of Fe. Given that the molar mass of Fe is 55.85 g/mol, we can calculate the theoretical mass of Fe produced from 0.339 mol of Fe2O3:
(0.339 mol Fe2O3) × (2 mol Fe/1 mol Fe2O3) × (55.85 g Fe/1 mol Fe) → Mass of Fe
This calculation should yield a result close to 11.7 g to confirm the statement as true. However, using the above information provided in the reference, if 0.013 moles of Fe is produced from 1.0 gram of Fe2O3, this scales to:
(0.339 mol Fe2O3) × (0.013 mol Fe/0.001 mol Fe2O3) × (55.85 g Fe/1 mol Fe) → Mass of Fe
Calculating the above gives us an expected theoretical mass of iron, which should be considered in determining the truth value of the statement. As the question does not provide the complete reaction and molar masses needed to reach a conclusion, it cannot be answered definitively as true or false without further information.