## TiCl4 (g) + 1 O2 (g) → TiO2 (s rutile) + 2 Cl2 (g)

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## Stoichiometry

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 TiCl4          Mass: g or Gas Volume: L O2             Mass: g or Gas Volume: L TiO2           Mass: g Cl2            Mass: g or Gas Volume: L Heat Released: kJ

## Enthalpy of Reaction

[1ΔHf(TiO2 (s rutile)) + 2ΔHf(Cl2 (g))] - [1ΔHf(TiCl4 (g)) + 1ΔHf(O2 (g))]
[1(-944.75) + 2(0)] - [1(-763.16) + 1(0)] = -181.59 kJ
-181.59 kJ     (exothermic)

## Entropy Change

[1ΔSf(TiO2 (s rutile)) + 2ΔSf(Cl2 (g))] - [1ΔSf(TiCl4 (g)) + 1ΔSf(O2 (g))]
[1(50.33) + 2(222.97)] - [1(354.8) + 1(205.03)] = -63.5600000000001 J/K
-63.56 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(TiO2 (s rutile)) + 2ΔGf(Cl2 (g))] - [1ΔGf(TiCl4 (g)) + 1ΔGf(O2 (g))]
[1(-889.52) + 2(0)] - [1(-726.76) + 1(0)] = -162.76 kJ
-162.76 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-162.64 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

3.2802350316e+028
This process is favorable at 25°C.