Determine the enthalpy change for the oxidation of iron, 2 Fe(s) + 3/2 O2(g) → Fe2O3(s) given the thermochemical equations below: Fe(s) + 3 H2O(liq) → Fe(OH)3(s) + 3/2 H2(g) ΔrH° = +160.9 kJ H2(g) + ½ O2(g) → H2O(liq) ΔrH° = -285.8 kJ Fe2O3(s) + 3 H2O(liq) → 2 Fe(OH)3(s) ΔrH° = +288.6 kJ a) +824.2 kJ b) -1648.4 kJ c) -824.2 kJ d) +1648.4 kJ
Determine the enthalpy change for the oxidation of iron, 2 Fe(s) + 3/2 O2(g) → Fe2O3(s) given the thermochemical equations below: Fe(s) + 3 H2O(liq) → Fe(OH)3(s) + 3/2 H2(g) ΔrH° = +160.9 kJ H2(g) + ½ O2(g) → H2O(liq) ΔrH° = -285.8 kJ Fe2O3(s) + 3 H2O(liq) → 2 Fe(OH)3(s) ΔrH° = +288.6 kJ a) +824.2 kJ b) -1648.4 kJ c) -824.2 kJ d) +1648.4 kJ
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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Determine the enthalpy change for the oxidation of iron,
2 Fe(s) + 3/2 O2(g) → Fe2O3(s)
given the thermochemical equations below:
Fe(s) + 3 H2O(liq) → Fe(OH)3(s) + 3/2 H2(g) ΔrH° = +160.9 kJ
H2(g) + ½ O2(g) → H2O(liq) ΔrH° = -285.8 kJ
Fe2O3(s) + 3 H2O(liq) → 2 Fe(OH)3(s) ΔrH° = +288.6 kJ
a) +824.2 kJ
b) -1648.4 kJ
c) -824.2 kJ
d) +1648.4 kJ
e) -1447.1 kJ
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