2 TiO2 (s rutile) + 3 C (s graphite) + 4 Cl2 (g) → 2 TiCl4 (g) + CO2 (g) + 2 CO (g)

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Stoichiometry

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 TiO2           Mass: g C              Mass: g Cl2            Mass: g or Gas Volume: L TiCl4          Mass: g or Gas Volume: L CO2            Mass: g or Gas Volume: L CO             Mass: g or Gas Volume: L Heat Released: kJ

Enthalpy of Reaction

[2ΔHf(TiCl4 (g)) + 1ΔHf(CO2 (g)) + 2ΔHf(CO (g))] - [2ΔHf(TiO2 (s rutile)) + 3ΔHf(C (s graphite)) + 4ΔHf(Cl2 (g))]
[2(-763.16) + 1(-393.51) + 2(-110.54)] - [2(-944.75) + 3(0) + 4(0)] = -251.41 kJ
-251.41 kJ     (exothermic)

Entropy Change

[2ΔSf(TiCl4 (g)) + 1ΔSf(CO2 (g)) + 2ΔSf(CO (g))] - [2ΔSf(TiO2 (s rutile)) + 3ΔSf(C (s graphite)) + 4ΔSf(Cl2 (g))]
[2(354.8) + 1(213.68) + 2(197.9)] - [2(50.33) + 3(5.69) + 4(222.97)] = 309.47 J/K
309.47 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(TiCl4 (g)) + 1ΔGf(CO2 (g)) + 2ΔGf(CO (g))] - [2ΔGf(TiO2 (s rutile)) + 3ΔGf(C (s graphite)) + 4ΔGf(Cl2 (g))]
[2(-726.76) + 1(-394.38) + 2(-137.28)] - [2(-889.52) + 3(0) + 4(0)] = -343.42 kJ
-343.42 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-343.68 kJ     (spontaneous)

Equilibrium Constant, K (at 298.15 K)

1.4720709516e+060
This process is favorable at 25°C.

Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 136.