When 50.0 g of iron(III) oxide reacts with carbon monoxide, 32.8 g of iron is produced. What is the percent yield of Fe for the reaction? (9.2, 9.3, 9.4, 9.5) Fe2O3(s) + 3CO(g) -> 2Fe(s) + 3CO2(g)
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The molar mass of Fe2O3 is approximately 159.69 g/mol and the molar mass of Fe is approximately 55.85 g/mol. From the balanced chemical equation, we can see that 1 mol of Fe2O3 produces 2 mol of Fe. So, if we start with 50.0 g of Fe2O3, we have 50.0 g / 159.69 Show more…
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Iron oxide can be reduced to the metal as follows: $$ \mathrm{Fe}_{2} \mathrm{O}_{3}(\mathrm{~s})+3 \mathrm{CO}(\mathrm{g}) \longrightarrow 2 \mathrm{Fe}(\mathrm{s})+3 \mathrm{CO}_{2}(\mathrm{~g}) $$ How many grams of iron can be obtained from $1.00 \mathrm{~kg}$ of the iron oxide? If $654 \mathrm{~g}$ Fe was obtained from the reaction, what was the percent yield?
Consider the extraction of iron from iron(III) oxide by charcoal $$2 \mathrm{Fe}_{2} \mathrm{O}_{3}(s)+3 \mathrm{C}(s) \longrightarrow 4 \mathrm{Fe}(s)+3 \mathrm{CO}_{2}(g)$$ When $12.5 \mathrm{~g}$ of $\mathrm{Fe}_{2} \mathrm{O}_{3}$ react with $2.6 \mathrm{~g}$ of $\mathrm{C}, 7.0 \mathrm{~g}$ of $\mathrm{Fe}$ is extracted. Determine the limiting reactant, theoretical yield of Fe and percent yield for the reaction
Iron oxide can be reduced to the metal as follows: $$\mathrm{Fe}_{2} \mathrm{O}_{3}(\mathrm{~s})+3 \mathrm{CO}(\mathrm{g}) \longrightarrow 2 \mathrm{Fe}(\mathrm{s})+3 \mathrm{CO}_{2}(\mathrm{~g})$$ Calculate the mass of iron that can be obtained from $1.00 \mathrm{~kg}$ of the iron oxide. If $654 \mathrm{~g}$ Fe was obtained from the reaction, calculate the percent yield.
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