## C12H22O11 (s sucrose) → 12 C (s graphite) + 11 H2O (g)

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Decomposition

## Stoichiometry

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 C12H22O11      Mass: g C              Mass: g H2O            Mass: g or Gas Volume: L Heat Released: kJ

## Enthalpy of Reaction

[12ΔHf(C (s graphite)) + 11ΔHf(H2O (g))] - [1ΔHf(C12H22O11 (s sucrose))]
[12(0) + 11(-241.82)] - [1(-2225.47)] = -434.55 kJ
-434.55 kJ     (exothermic)

## Entropy Change

[12ΔSf(C (s graphite)) + 11ΔSf(H2O (g))] - [1ΔSf(C12H22O11 (s sucrose))]
[12(5.69) + 11(188.72)] - [1(360.24)] = 1783.96 J/K
1,783.96 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[12ΔGf(C (s graphite)) + 11ΔGf(H2O (g))] - [1ΔGf(C12H22O11 (s sucrose))]
[12(0) + 11(-228.59)] - [1(-1544.65)] = -969.84 kJ
-969.84 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-966.44 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

8.280779136e+169
This process is favorable at 25°C.

## Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 216.
Zumdahl, Steven and Zumdahl, Susan A. Chemistry 9th ed.; Brooks/Cole: Belmont, CA, 2014; p 131.