Fe (s alpha) + 2 HCl (aq) → FeCl2 (aq) + 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
FeCl2          Mass: g  or Solution Volume: mL of Concentration: mol/L
H2             Mass: g  or Gas Volume: L

Enthalpy of Reaction

[1ΔHf(FeCl2 (aq)) + 1ΔHf(H2 (g))] - [1ΔHf(Fe (s alpha)) + 2ΔHf(HCl (aq))]
[1(-423.42) + 1(0)] - [1(0) + 2(-167.15)] = -89.12 kJ
-89.12 kJ     (exothermic)

Entropy Change

[1ΔSf(FeCl2 (aq)) + 1ΔSf(H2 (g))] - [1ΔSf(Fe (s alpha)) + 2ΔSf(HCl (aq))]
[1(-24.69) + 1(130.59)] - [1(27.28) + 2(56.48)] = -34.34 J/K
-34.34 J/K     (decrease in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(FeCl2 (aq)) + 1ΔGf(H2 (g))] - [1ΔGf(Fe (s alpha)) + 2ΔGf(HCl (aq))]
[1(-341.37) + 1(0)] - [1(0) + 2(-131.25)] = -78.87 kJ
-78.87 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-78.88 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

65795325228318.5
This process is favorable at 25°C.