## 2 Fe (s alpha) + 6 HCl (aq) → 2 FeCl3 (aq) + 3 H2 (g)

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## Reaction Type:

Single displacement/Oxidation-reduction

## Stoichiometry

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 Fe             Mass: g HCl            Mass: g or Solution Volume: mL of Concentration: mol/L FeCl3          Mass: g H2             Mass: g or Gas Volume: L Heat Released: kJ

## Enthalpy of Reaction

[2ΔHf(FeCl3 (aq)) + 3ΔHf(H2 (g))] - [2ΔHf(Fe (s alpha)) + 6ΔHf(HCl (aq))]
[2(-549.98) + 3(0)] - [2(0) + 6(-167.15)] = -97.0599999999999 kJ
-97.06 kJ     (exothermic)

## Entropy Change

[2ΔSf(FeCl3 (aq)) + 3ΔSf(H2 (g))] - [2ΔSf(Fe (s alpha)) + 6ΔSf(HCl (aq))]
[2(-146.45) + 3(130.59)] - [2(27.28) + 6(56.48)] = -294.57 J/K
-294.57 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(FeCl3 (aq)) + 3ΔGf(H2 (g))] - [2ΔGf(Fe (s alpha)) + 6ΔGf(HCl (aq))]
[2(-398.35) + 3(0)] - [2(0) + 6(-131.25)] = -9.20000000000005 kJ
-9.20 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-9.23 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

40.912870495
This process is favorable at 25°C.