a) Given the balanced reaction between ferric oxide and carbon expressed as:
[tex]Fe_2O_3+3C\rightarrow3CO+2Fe[/tex]Determine the moles of CO
[tex]\begin{gathered} \text{Moles of CO=}\frac{Mass\text{ of CO}}{Molar\text{ mass of CO}} \\ \text{Moles of CO}=\frac{15g}{12+16} \\ \text{Moles of CO}=\frac{15}{28} \\ \text{Moles of CO}=0.536\text{moles} \end{gathered}[/tex]Based on stochiometry, 1 mole of ferric oxide produce 3 moles of CO, hence 0.536 moles of CO will produce:
[tex]\begin{gathered} \text{Moles of Fe}_2O_3=\frac{0.536\times1}{3} \\ \text{Moles of Fe}_2O_3=0.179\text{moles} \end{gathered}[/tex]Determine the mass of Fe₂O₃
[tex]\begin{gathered} \text{Mass}=\text{Moles}\times\text{molar mass} \\ \text{Mass of Fe}_2O_3=0.179\times\lbrack2(55.845)+3(16)\rbrack \\ \text{Mass of Fe}_2O_3=0.179\times(159.69) \\ \text{Mass of Fe}_2O_3=28.58\text{grams} \end{gathered}[/tex]Hence the amount of mass of Ferric Oxide that is needed to produce 15g of CO is 28.58grams.
b) From the given reaction, carbon is known to be oxidized to produce carbon monoxide while ferric oxide is reduced to produce Fe. Hence the type of reaction between Ferric oxide and carbon as shown is a Redox reaction