Question

2. Combining 0.242 mol Fe2O3 with excess carbon produced 10.2 g Fe.

Answer 1

actual yield = 0.182 mole

theoretical yield : 0.484 mole

percentage mole(% yield)=37.6%

Further explanation

Percent yield is the comparison of the amount of product obtained from a reaction with the amount you calculated

General formula:

Percent yield = (Actual yield / theoretical yield )x 100%

An actual yield is the amount of product actually produced by the reaction. A theoretical yield is the amount of product that you calculate from the reaction equation according to the product and reactant coefficients

Reaction

Fe₂O₃+3C⟶2Fe+3CO

a. actual yield of Fe mole

10.2 g produced

$\tt mol~Fe=\dfrac{10.2}{56}=0.182$

b. percentage mole and theoretical yield

0.242 mol Fe₂O₃ = 2 x 0.242 mol Fe = 0.484 mol (theoretical yield)

percentage yieldpercentage mole)

$\tt \dfrac{0.182}{0.484}=0.376=37.6\%$