## 3 TiO2 (s rutile) + 4 BrF3 (ℓ) → 3 TiF4 (s) + 2 Br2 (ℓ) + 3 O2 (g)

Back to reactions list

## Stoichiometry

Enter a mass or volume in one of the boxes below. Upon hitting submit, the stoichiometric equivalents will be calculated for the remaining reactants and products. All gases are assumed to be at STP.

 TiO2           Mass: g BrF3           Mass: g TiF4           Mass: g Br2            Mass: g O2             Mass: g or Gas Volume: L Heat Released: kJ

## Enthalpy of Reaction

[3ΔHf(TiF4 (s)) + 2ΔHf(Br2 (ℓ)) + 3ΔHf(O2 (g))] - [3ΔHf(TiO2 (s rutile)) + 4ΔHf(BrF3 (ℓ))]
[3(-1649.33) + 2(0) + 3(0)] - [3(-944.75) + 4(-300.83)] = -910.42 kJ
-910.42 kJ     (exothermic)

## Entropy Change

[3ΔSf(TiF4 (s)) + 2ΔSf(Br2 (ℓ)) + 3ΔSf(O2 (g))] - [3ΔSf(TiO2 (s rutile)) + 4ΔSf(BrF3 (ℓ))]
[3(133.97) + 2(152.23) + 3(205.03)] - [3(50.33) + 4(178.24)] = 457.51 J/K
457.51 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[3ΔGf(TiF4 (s)) + 2ΔGf(Br2 (ℓ)) + 3ΔGf(O2 (g))] - [3ΔGf(TiO2 (s rutile)) + 4ΔGf(BrF3 (ℓ))]
[3(-1559.38) + 2(0) + 3(0)] - [3(-889.52) + 4(-240.58)] = -1047.26 kJ
-1,047.26 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-1046.83 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

3.035450079e+183
This process is favorable at 25°C.

## Reference(s):

Kotz, John C. and Treichel, Paul. Chemistry & Chemical Reactivity 4th ed.; Thomson Brooks/Cole: Belmont, CA, 1999; p 166.
Kotz, John C., Treichel, Paul, and Weaver, Gabriela. Chemistry & Chemical Reactivity 6th ed.; Thomson Brooks/Cole: Belmont, CA, 2006; p 161.