CH4 (g methane) + 1 H2O (g) → CO (g) + 3 H2 (g)

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Stoichiometry

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Heat Added: kJ
CH4            Mass: g
H2O            Mass: g  or Gas Volume: L
CO             Mass: g  or Gas Volume: L
H2             Mass: g  or Gas Volume: L

Enthalpy of Reaction

[1ΔHf(CO (g)) + 3ΔHf(H2 (g))] - [1ΔHf(CH4 (g methane)) + 1ΔHf(H2O (g))]
[1(-110.54) + 3(0)] - [1(-74.85) + 1(-241.82)] = 206.13 kJ
206.13 kJ     (endothermic)

Entropy Change

[1ΔSf(CO (g)) + 3ΔSf(H2 (g))] - [1ΔSf(CH4 (g methane)) + 1ΔSf(H2O (g))]
[1(197.9) + 3(130.59)] - [1(186.27) + 1(188.72)] = 214.68 J/K
214.68 J/K     (increase in entropy)

Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(CO (g)) + 3ΔGf(H2 (g))] - [1ΔGf(CH4 (g methane)) + 1ΔGf(H2O (g))]
[1(-137.28) + 3(0)] - [1(-50.84) + 1(-228.59)] = 142.15 kJ
142.15 kJ     (nonspontaneous)

From ΔG = ΔH - TΔS:
142.12 kJ     (nonspontaneous)

Equilibrium Constant, K (at 298.15 K)

1.2445482331e-025
This process is not favorable at 25°C.

Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 226.
Kotz, John C., Treichel, Paul, and Weaver, Gabriela. Chemistry & Chemical Reactivity 6th ed.; Thomson Brooks/Cole: Belmont, CA, 2006; p 167.

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