2 Cr (s) + 3 Cl2 (g) → 2 CrCl3 (s)

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Cr             Mass: g
Cl2            Mass: g  or Gas Volume: L
CrCl3          Mass: g
Heat Released: kJ

Entropy Change

[2ΔSf(CrCl3 (s))] - [2ΔSf(Cr (s)) + 3ΔSf(Cl2 (g))]
[2(123)] - [2(23.62) + 3(222.97)] = -470.15 J/K
-470.15 J/K     (decrease in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(CrCl3 (s))] - [2ΔGf(Cr (s)) + 3ΔGf(Cl2 (g))]
[2(-486.1)] - [2(0) + 3(0)] = -972.2 kJ
-972.20 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-972.82 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

This process is favorable at 25°C.


Kotz, John C. and Treichel, Paul. Chemistry & Chemical Reactivity 4th ed.; Thomson Brooks/Cole: Belmont, CA, 1999; p 173.
Kotz, John C., Treichel, Paul, and Weaver, Gabriela. Chemistry & Chemical Reactivity 6th ed.; Thomson Brooks/Cole: Belmont, CA, 2006; p 166.

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