Answered: Fe(s) + O2(g) Fe2O3(s) If 1.05 g of…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

Fe(s) + O₂(g) Fe₂O₃(s)

If 1.05 g of iron is heated and placed in a bottle containing 0.0219 mol of oxygen gas, what mass of iron(III) oxide is produced?

Expert Solution

Step 1

To calculate the mass of iron (III) oxide produced we would proceed as :

First write the balanced chemical reaction between iron and oxygen to produce iron (III) oxide.
Then we need to calculate moles of iron using given mass and its molar mass.
Then we need to determine limiting reagent. For this we calculate moles of iron(III) oxide produced by both reactants separately using their moles and mole ratio. The reactants which produces less moles will be the limiting reagent.
To calculate the mass of product , we use the moles of product produced by limiting reagent. So mass can be calculated using the moles and molar mass.

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