## Fe2O3 (s hematite) + 3 H2SO4 (aq) → Fe2(SO4)3 (aq) + 3 H2O (ℓ)

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## Reaction Type:

Double Displacement

## Stoichiometry

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 Fe2O3          Mass: g H2SO4          Mass: g or Solution Volume: mL of Concentration: mol/L Fe2(SO4)3      Mass: g H2O            Mass: g Heat Released: kJ

## Enthalpy of Reaction

[1ΔHf(Fe2(SO4)3 (aq)) + 3ΔHf(H2O (ℓ))] - [1ΔHf(Fe2O3 (s hematite)) + 3ΔHf(H2SO4 (aq))]
[1(-2824.87) + 3(-285.83)] - [1(-824.25) + 3(-909.27)] = -130.3 kJ
-130.30 kJ     (exothermic)

## Entropy Change

[1ΔSf(Fe2(SO4)3 (aq)) + 3ΔSf(H2O (ℓ))] - [1ΔSf(Fe2O3 (s hematite)) + 3ΔSf(H2SO4 (aq))]
[1(-571.54) + 3(69.91)] - [1(87.4) + 3(20.08)] = -509.45 J/K
-509.45 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(Fe2(SO4)3 (aq)) + 3ΔGf(H2O (ℓ))] - [1ΔGf(Fe2O3 (s hematite)) + 3ΔGf(H2SO4 (aq))]
[1(-2243.09) + 3(-237.18)] - [1(-742.24) + 3(-744.63)] = 21.5000000000005 kJ
21.50 kJ     (nonspontaneous)

From ΔG = ΔH - TΔS:
21.59 kJ     (nonspontaneous)

## Equilibrium Constant, K (at 298.15 K)

0.00017106193289
This process is not favorable at 25°C.

## Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 217.