## Fe2O3 (s hematite) + 6 HCl (aq) → 2 FeCl3 (aq) + 3 H2O (ℓ)

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## Stoichiometry

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 Fe2O3          Mass: g HCl            Mass: g or Solution Volume: mL of Concentration: mol/L FeCl3          Mass: g H2O            Mass: g Heat Released: kJ

## Enthalpy of Reaction

[2ΔHf(FeCl3 (aq)) + 3ΔHf(H2O (ℓ))] - [1ΔHf(Fe2O3 (s hematite)) + 6ΔHf(HCl (aq))]
[2(-549.98) + 3(-285.83)] - [1(-824.25) + 6(-167.15)] = -130.3 kJ
-130.30 kJ     (exothermic)

## Entropy Change

[2ΔSf(FeCl3 (aq)) + 3ΔSf(H2O (ℓ))] - [1ΔSf(Fe2O3 (s hematite)) + 6ΔSf(HCl (aq))]
[2(-146.45) + 3(69.91)] - [1(87.4) + 6(56.48)] = -509.45 J/K
-509.45 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(FeCl3 (aq)) + 3ΔGf(H2O (ℓ))] - [1ΔGf(Fe2O3 (s hematite)) + 6ΔGf(HCl (aq))]
[2(-398.35) + 3(-237.18)] - [1(-742.24) + 6(-131.25)] = 21.5 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 94.