## 2 CH4 (g methane) + 1 O2 (g) → 2 CO (g) + 4 H2 (g)

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## Stoichiometry

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 CH4            Mass: g O2             Mass: g or Gas Volume: L CO             Mass: g or Gas Volume: L H2             Mass: g or Gas Volume: L Heat Released: kJ

## Enthalpy of Reaction

[2ΔHf(CO (g)) + 4ΔHf(H2 (g))] - [2ΔHf(CH4 (g methane)) + 1ΔHf(O2 (g))]
[2(-110.54) + 4(0)] - [2(-74.85) + 1(0)] = -71.38 kJ
-71.38 kJ     (exothermic)

## Entropy Change

[2ΔSf(CO (g)) + 4ΔSf(H2 (g))] - [2ΔSf(CH4 (g methane)) + 1ΔSf(O2 (g))]
[2(197.9) + 4(130.59)] - [2(186.27) + 1(205.03)] = 340.59 J/K
340.59 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(CO (g)) + 4ΔGf(H2 (g))] - [2ΔGf(CH4 (g methane)) + 1ΔGf(O2 (g))]
[2(-137.28) + 4(0)] - [2(-50.84) + 1(0)] = -172.88 kJ
-172.88 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-172.93 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

1.9451401966e+030
This process is favorable at 25°C.

## Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 226.