Answer :
Answer:
483.07 grams
Explanations:
The reaction between Iron (III) oxide and carbon to produce solid iron and carbon monoxide is given as
[tex]Fe_2O_3+3C\rightarrow2Fe+3CO[/tex]Determine the moles of Iron(III) oxide
[tex]\begin{gathered} moles\text{ of Fe}_2O_3=\frac{mass}{molar\text{ mass}} \\ moles\text{ of Fe}_2O_3=\frac{690.67}{159.69} \\ moles\text{ of Fe}_2O_3=4.325moles \end{gathered}[/tex]According to stoichiometry, 1 mole of Iron(III)oxide produced 2 moles of Iron. The moles of Iron required is expressed as:
[tex]\begin{gathered} mole\text{ of Fe}=2\times4.325moles \\ mole\text{ of Fe}=8.65moles \end{gathered}[/tex]Determine the mass of Iron produced
[tex]\begin{gathered} Mass\text{ of Fe}=mole\times molar\text{ mass} \\ Mass\text{ of Fe}=8.65\times55.845 \\ Mass\text{ of Fe}=483.07grams \end{gathered}[/tex]Hence the mass of iron that can be produced is 483.07 grams