Question

Combining 0.336 mol Fe₂O3, with excess carbon produced 17.5 g Fe.Fe₂O3 + 3C….>2 Fe + 3 COWhat 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 actual yield of iron in moles = 0.313 mol

The theoretical yield of iron in moles = 0.672 mol

The percent yield = 46.58%

Step-by-step explanation

Given:

Moles of Fe₂O₃ that react = 0.336 mol

Mass of Fe produced = 17.5 g

Equation: Fe₂O₃ + 3C → 2Fe + 3CO

What to find:

i. The actual yield of iron in moles.

ii. The theoretical yield of iron in moles.

iii. The percent yield.

Step-by-step solution:

i. The actual yield of iron in moles.

From the given information; the actual yield of Fe in grams is 17.5 g.

So, the actual yield in moles can be determined by converting grams to mole using the mole formula.

`Moles=\frac{Mass}{Molar\text{ }mass}`

Using the periodic table, the molar mass of Fe = 55.845 g/mol

`Moles=\frac{17.5g}{55.845g\text{/}mol}=0.313\text{ }mol`

Therefore, the actual yield of iron in moles is 0.313 mol.

ii. The theoretical yield of iron in moles.

Using the mole ratio Fe₂O₃ and Fe, and the given moles of Fe₂O₃; theoretical yield of Fe in moles is calculated as follows:

`\begin{gathered} 1\text{ }mol\text{ }Fe₂O₃=2\text{ }mol\text{ }Fe \\ \\ 0.336\text{ }mol\text{ }Fe₂O₃=x \\ \\ x=\frac{0.336\text{ }mol\text{ }Fe₂O₃}{1\text{ }mol\text{ }Fe₂O₃}*2\text{ }mol\text{ }Fe \\ \\ x=0.672\text{ }mol\text{ }Fe \end{gathered}`

Thus, the theoretical yield of iron in moles is 0.672 mol.

iii. The percent yield.

The percent yield is calculated using the formula:

`Percent\text{ }yield=\frac{Actual\text{ }yield}{Theoretical\text{ }yield}*100\%`

Putting the actual yield = 0.313 mol and the theoretical yield = 0.672 mol into the formula, we have the percent yield to be equal:

`\begin{gathered} Percent\text{ }yield=\frac{0.313\text{ }mol}{0.672\text{ }mol}*100\% \\ \\ Percent\text{ }yield.=46.58\% \end{gathered}`

The percent yield is 46.58%