2) The oxidation of iron is described by the following reaction: 4 Fe(s) + 3 O2(g) → 2 Fe203(s) a) How many moles Fe are needed to produce 124 moles of Fe2O3? b) How many grams of Fe2O3 are produced when 82.8g of Fe react with as much 02 as needed? total) C c) How many grams of Fe203 are produced when 125g of Fe react with 125g of O2 (theoretical yield)? Which one of the reactants is the limiting reagent?

2) The oxidation of iron is described by the following reaction: 4 Fe(s) + 3 O2(g) → 2 Fe203(s) a) How many moles Fe are needed to produce 124 moles of Fe2O3? b) How many grams of Fe2O3 are produced when 82.8g of Fe react with as much 02 as needed? total) C c) How many grams of Fe203 are produced when 125g of Fe react with 125g of O2 (theoretical yield)? Which one of the reactants is the limiting reagent?

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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so this whole question is split into four parts but it's technically one whole problem. 11). Answer the following for the balanced equation: Fe203 + 3CO -----> 2Fe + 3CO2: A) What is the theoretical yield of the first product if 20.0 grams of the first reactant and 20.0 grams of the second reactant are reacted? B) Which reactant is the limiting reactant? C) How many grams of the excess reactant are reacted? D) How many grams of the excess reactant are left…