Steam reforming of methane(CH4) produces \"synthesis gas,\' a mixture of carbon

Question

Steam reforming of methane(CH4) produces "synthesis gas,' a mixture of carbon monoxide gas and hydrogen gas, which is the starting point for many important industrial chemical syntheses. An industrial chemist studying this reaction fills a 5.0 L flask with 1.0 atm of methane gas and 1.7 atm of water vapor at 43.0C. He then raises the temperature, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 2.7 atm. Calculate the pressure equilibrium constant for the steam reforming of methane at the final temperature of the mixture. Round your answer to 2 significant digits I Don't Know Submit

Explanation / Answer

CH4 + H2O = CO + H2

balance

CH4 + H2O = CO + 3H2

P-CH4 = 1 atm

P-H2O = 2.7

P-CO = 0

P-H2 = 0

in equilibrium

P-CH4 = 1 - x

P-H2O = 2.7 - x

P-CO = 0 + x

P-H2 = 0 +3x

and we know that in equilibrium, H2 gas = 2.7 atm

P-H2 = 0 +3x = 2.7

x = 2.7/3 = 0.9 atm

so

P-CH4 = 1 - x = 1-0.90 = 0.10

P-H2O = 2.7 - x = 2.7-0.90 = 1.8 atm

P-CO = 0 + x = 0.90

P-H2 = 0 +3x = 2.7 atm

Kp = P-CO * P-H2^3 / (P-CH4)(P-H2O)

Kp = (0.90)(2.7^3) / (0.10*1.8)

Kp = 98.415

Kp = 9.84*10^1

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