Question

Combining 0.284 mol Fe 2 O 3 with excess carbon produced 18.6 g Fe . Fe 2 O 3 + 3 C ⟶ 2 Fe + 3 CO What is the actual yield of iron in moles?

actual yield:

What is the theoretical yield of iron in moles? theoretical yield:

What is the percent yield? percent yield:

Answer 1

The problem based on limiting reagent concept, in this first we want to proceed as reaction balanced or not, next step is what is limiting reagent by knowing a clear definition of it, next calculate theoretical, actual yield, and proceed for final step as percent yield.

Balanced Reaction is Te O₂ +30 2 Fe+300 i molef Te, 3 reacts with 3 molesof Carbon Carbon is in excess, and out of Tegos, C, Carbon excess means Te, 03 E8 En limiting reagent which is present in limited quantity, deude the product formation: Fe₂O3 + 3 C ~ 2 Fe + 300 i moleef 1903 reacts to produce zmolesof te Given 18.6g of Fe formed No of moles of Fe = 18-6 = 0.333. 5585 moles 0.284 molof Feog reacts to produce moles of te 2 0.284 X2 = 0.568 moles Theoritical Acizel yield of tron = 0-568 moles p Altural Theri cal gend of iron = 0.38 3 moles Yield percent yield = xloo @ Actual field Theoriticalyield 0.333 x 100 0.568 = 58.6.1.