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To make pure iron metal from its ore, iron(III) oxide must react with carbon monoxide. The...

Question:

To make pure iron metal from its ore, iron(III) oxide must react with carbon monoxide. The products of this reaction are iron metal and carbon dioxide gas. The balanced chemical equation for this reaction is given below.

{eq}Fe_2O_3 + 3CO \to 2Fe + 3CO_2 {/eq}

Suppose {eq}1.4 \times 10^3 {/eq} moles of iron(III) oxide reacts with a sufficient amount of carbon monoxide.

a. How many moles of pure iron metal will be produced?

b. How many moles of carbon dioxide will be released into the air?

c. How many moles of carbon monoxide will be required to fully change the ore into its metal?

Steel:

Pure iron is often mixed with other elements to produce alloys. Alloys tend to strengthen metals and can sometimes provide protection against rusting. For example, steel is an alloy primarily of carbon and iron.

Answer and Explanation:

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We are told that {eq}\rm 1.4 \times 10^3 {/eq} moles of iron(III) oxide ({eq}\rm Fe_2O_3 {/eq}) react in the following reaction:


{eq}\rm Fe_2O_3...

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Mole-to-Mole Ratios and Calculations of a Chemical Equation

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Chapter 9 / Lesson 2
155K

Learn about the mole ratio. Understand the definition of mole ratio, how to find mole ratio in stoichiometry, and see examples of using mole ratio in problems.


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