The decomposition of methane into carbon is desired at atmospheric pressure for

Question

The decomposition of methane into carbon is desired at atmospheric pressure for a starting mole ratio of one with nitrogen (to reduce the hazard of uncontrolled combustion from possible oxygen leakage into the process) at T = 650 degree C. Calculate the equilibrium constant for the above reaction equation. Compute all compositions at the final extent of reaction. How much of the methane is converted at equilibrium'? Does any reaction occur at a room temperature of 298 K, where Delta g degree 298 = 50.5 kJ/mol? If not, show mathematically why this is true If so, show mathematically why. How else might the equilibrium extent of reaction be increased for this reaction, and why?

Explanation / Answer

deltaG = -RT * ln(K)

-11100J = -8.315J/mole-K x (650+273)K x ln(K)

1.4463 = ln(K)

e^1.4463 = k

k = 4.247

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