2 Fe (s alpha) + 3 Cl2 (g) → 2 FeCl3 (s)

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Reaction Type:

Synthesis

Stoichiometry

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Fe             Mass: g
Cl2            Mass: g  or Gas Volume: L
FeCl3          Mass: g

Enthalpy of Reaction

[2ΔHf(FeCl3 (s))] - [2ΔHf(Fe (s alpha)) + 3ΔHf(Cl2 (g))]
[2(-399.49)] - [2(0) + 3(0)] = -798.98 kJ
-798.98 kJ     (exothermic)

Entropy Change

[2ΔSf(FeCl3 (s))] - [2ΔSf(Fe (s alpha)) + 3ΔSf(Cl2 (g))]
[2(142.26)] - [2(27.28) + 3(222.97)] = -438.95 J/K
-438.95 J/K     (decrease in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(FeCl3 (s))] - [2ΔGf(Fe (s alpha)) + 3ΔGf(Cl2 (g))]
[2(-334.05)] - [2(0) + 3(0)] = -668.1 kJ
-668.10 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-668.11 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

1.12867484517649E+117
This process is favorable at 25°C.

Reference(s):

Kotz, John C., Treichel, Paul, and Weaver, Gabriela. Chemistry & Chemical Reactivity 6th ed.; Thomson Brooks/Cole: Belmont, CA, 2006; p 144.

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