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}

Answer and Explanation: 1

Become a Study.com member to unlock this answer!

View 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...

See full answer below.


Learn more about this topic:

Loading...
How to Calculate Percent Yield: Definition, Formula & Example

from

Chapter 10 / Lesson 15
330K

What is percent yield? Learn the definition and formula of percent yield. Learn about actual and theoretical yields. See examples of percent yield calculations.


Related to this Question

Explore our homework questions and answers library