# Iron(III) oxide reacts with carbon monoxide to produce iron and carbon dioxide. Fe2O3(s) + 3CO(g)...

## Question:

Iron(III) oxide reacts with carbon monoxide to produce iron and carbon dioxide:

{eq}\rm Fe_2O_3(s) + 3CO(g) \to 2Fe(s) + 3CO_2(g) {/eq}

What is the percent yield for iron if the reaction of 70.0 grams of iron(III) oxide produces 38.0 grams of iron?

## Percent Yield:

The percent yield of a chemical reaction is usually less than a hundred percent due to reaction factors, such as secondary or incomplete reactions or incomplete recovery of the final product. If the value of percent yield is more than a hundred percent, it often means that impurities are present in the sample. The general equation for calculating percent yield for a reaction is:

{eq}\rm \%\;Yield = \dfrac{Actual\;Yield}{Theoretical\;Yield} \times 100\% {/eq}

Become a Study.com member to unlock this answer!

Given Data:

• Mass of iron oxide = 70.0 g
• Mass of iron = 38.0 g
• Molar mass of iron oxide = 159.69 g/mol
• Molar mass of iron = 55.845 g/mol

The given...