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The following thermochemical equation is for the reaction of iron(III) oxide(s) with hydrogen(g) to form iron(s) and water(g). Fe2O3(s) + 3H2(g)2Fe(s) + 3H2O(g)     H = 98.8 kJ When 44.6 grams of iron(III) oxide(s) react with excess hydrogen(g), kJ of energy are

The following thermochemical equation is for the reaction of iron(III) oxide(s) with hydrogen(g) to form iron(s) and water(g). Fe2O3(s) + 3H2(g)2Fe(s) + 3H2O(g)     H = 98.8 kJ When 44.6 grams of iron(III) oxide(s) react with excess hydrogen(g), kJ of energy are

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter8: Thermochemistry
Section: Chapter Questions
Problem 36QAP: Given the following thermochemical equations: 4B(s)+3O2(g)2B2O3(s)H=2543.8kJ H2(g)+12...
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The following thermochemical equation is for the reaction of iron(III) oxide(s) with hydrogen(g) to form iron(s) and water(g).

Fe2O3(s)

      +

3H2(g)2Fe(s)

      +

3H2O(g)

          H =

98.8

    kJ

When 44.6 grams of iron(III) oxide(s) react with excess hydrogen(g), kJ of energy are

 

.

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