A gaseous mixture of 30 percent (by mole fraction) methane
Chapter 16, Problem 17P(choose chapter or problem)
A gaseous mixture of 30 percent (by mole fraction) methane and 70 percent carbon dioxide is heated at \(1 \mathrm{~atm}\) pressure to \(1200 \mathrm{~K}\). What is the equilibrium composition (by mole fraction) of the resulting mixture? The natural logarithm of the equilibrium constant for the reaction \(\mathrm{C}+2 \mathrm{H}_{2} \rightleftharpoons \mathrm{CH}_{4}\) at \(1200 \mathrm{~K}\) is 4.147.
Equation Transcription:
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Text Transcription:
1 atm
1200 K
C+2H_2 leftrightharpoons CH_4
1200 K
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