At 3000K and 8bar, methane (CH4) reacts with the stoichiometric amount of pure oxygen according to...

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At 3000K and 8bar, methane (CH4) reacts with the stoichiometric amount of pure oxygen according to CO₂ + 2 H₂O. The chemical constants for the following reactions are given (all at 3000K): CH₂ + 2 O₂ 2 H₂+ O₂ 2 H₂0 with K(T) = 484.9 1/bar C + 2 H₂ ⇒ CH₂ with K,(7) 9.685 1/(bar)² C+0₂ ⇒ CO₂ with K,(7) 15.87 1/bar a) Determine the chemical constant for the overall reaction b) Set-up all equations necessary to determine the mole fraction of CH, in equilibrium. Hint: number of unknowns must equal number of equations. At 3000K and 8bar, methane (CH4) reacts with the stoichiometric amount of pure oxygen according to CO₂ + 2 H₂O. The chemical constants for the following reactions are given (all at 3000K): CH₂ + 2 O₂ 2 H₂+ O₂ 2 H₂0 with K(T) = 484.9 1/bar C + 2 H₂ ⇒ CH₂ with K,(7) 9.685 1/(bar)² C+0₂ ⇒ CO₂ with K,(7) 15.87 1/bar a) Determine the chemical constant for the overall reaction b) Set-up all equations necessary to determine the mole fraction of CH, in equilibrium. Hint: number of unknowns must equal number of equations.

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Given Temperature T 3000 K Pressure P 1 bar Reactions CH4 202 CO2 2H2O 2H2 O2 2H2O K... View the full answer