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

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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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