   Chapter 4, Problem 1PS

Chapter
Section
Textbook Problem

The reaction of iron(III) oxide with aluminum to give molten iron is known as the thermite reaction (page 172).Fe2O3(s) + 2 Al(s) → 2 Fe(l) + Al2O3(s)What amount of Al, in moles, is needed for complete reaction with 3.0 mol of Fe2O3? What mass of Fe, in grams, can be produced?

Interpretation Introduction

Interpretation:

From the given reaction the amount of Aluminum in moles needed for complete the reaction with 3.0molofFe2O3 and the mass of Fe produced in grams should be determined.

Concept introduction:

• Numberofmole=GivenmassofthesubstanceMolarmass
• The molar mass of an element or compound is the mass in grams of 1 mole of that substance, and it is expressed in the unit of grams per mol (g/mol).
• For chemical reaction balanced chemical reaction equation established in accordance with the Law of conservation of mass.
• Stoichiometric factor is a relationship between reactant and product which is obtained from the balanced chemical equation for a particular reaction.

6.0 Mole aluminum is needed for complete the reaction with 3.0molofFe2O3 335.04g of Fe produced in the given reaction.

Explanation

Balanced chemical equation for the given reaction is,

Fe2O3(s)+2Al(s)2Fe(l)+Al2O3(s)

Using the stoichiometric factor calculating the amount of Aluminum required based on the amount of Fe2O3 as follows,

The amount of Aluminum in moles needed for complete the reaction with 3.0molofFe2O3

3.0molFe2O3×2molAl1molFe2O3=6molAl

The amount of Fe in gram produced in the given reaction determined as follows,

3.0molFe2O3×2molFe1molFe2O3×55.84gFe1molFe=335.04gFe

Therefore amount of Fe in gram produced in the given reaction is 335.04g.

Conclusion

The amount of Aluminum in moles needed for complete the reaction with and the mass of Fe produced in gram was determined.

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