1. Calculate the number of moles in each of the following samples. Show your work. (a) 150.0 g of Fe2O3 (b) 2.50 x 1021 molecules of ethanol, C2H,OH 2. Iron oxide ore, Fe,O4 yield elemental iron when heated to a very high temperature with carbon monoxide. The equation for the chemical process is Fe(s) CO2(g) Fe2O3(s) CO(g) (a) Balance the chemical equation. (b) How many moles of elemental iron can be produced by complete reaction of 75 moles of iron ore(Fe304)? Show your work.

1. Calculate the number of moles in each of the following samples. Show your work. (a) 150.0 g of Fe2O3 (b) 2.50 x 1021 molecules of ethanol, C2H,OH 2. Iron oxide ore, Fe,O4 yield elemental iron when heated to a very high temperature with carbon monoxide. The equation for the chemical process is Fe(s) CO2(g) Fe2O3(s) CO(g) (a) Balance the chemical equation. (b) How many moles of elemental iron can be produced by complete reaction of 75 moles of iron ore(Fe304)? Show your work.

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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