## C (s graphite) + 1 O2 (g) → CO2 (g)

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Synthesis

## Stoichiometry

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 C              Mass: g O2             Mass: g or Gas Volume: L CO2            Mass: g or Gas Volume: L Heat Released: kJ

## Enthalpy of Reaction

[1ΔHf(CO2 (g))] - [1ΔHf(C (s graphite)) + 1ΔHf(O2 (g))]
[1(-393.51)] - [1(0) + 1(0)] = -393.51 kJ
-393.51 kJ     (exothermic)

## Entropy Change

[1ΔSf(CO2 (g))] - [1ΔSf(C (s graphite)) + 1ΔSf(O2 (g))]
[1(213.68)] - [1(5.69) + 1(205.03)] = 2.96000000000001 J/K
2.96 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(CO2 (g))] - [1ΔGf(C (s graphite)) + 1ΔGf(O2 (g))]
[1(-394.38)] - [1(0) + 1(0)] = -394.38 kJ
-394.38 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-394.39 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

1.2480479034e+069
This process is favorable at 25°C.

## Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; pp 202, 204, 224.