What is the theoretical yield of iron (55.845 g/mol) when 10.0 g Fe ₂O₃ (159.69 g/mol) reacts with excess carbon (12.01 g/mol) ?
2 Fe₂O₃ (s) + 3 C(s) $\rightarrow$ 4 Fe(s) + 3 CO₂ (g)

Question

What is the theoretical yield of iron (55.845 g/mol) when 10.0 g Fe ₂O₃ (159.69 g/mol) reacts with excess carbon (12.01 g/mol)? 2 Fe₂O₃ (s) + 3 C(s) $\rightarrow$ 4 Fe(s) + 3 CO₂ (g)

Quizplus · Accepted Answer

The reaction shows that 2 moles of FeS₂ (pyrite) produce 4 moles of iron (Fe). First, calculate the moles of FeS₂ used: 10.0 g / 159.69 g/mol = 0.0626 mol. Since the reaction produces twice as many moles of Fe as FeS₂ used, the moles of Fe produced are 2 * 0.0626 mol = 0.1252 mol. The mass of Fe produced is then 0.1252 mol * 55.845 g/mol = 6.99 g.

What Is the Theoretical Yield of Iron (55 →\rightarrow→ 4 Fe(s) + 3 CO2 (G) A)3

What Is the Theoretical Yield of Iron (55 $\rightarrow$ 4 Fe(s) + 3 CO₂ (G)
A)3