KINETICS AND EQUILDBRIUM Calculating an equilibrium constant from a partial equi

Question

KINETICS AND EQUILDBRIUM Calculating an equilibrium constant from a partial equilib. 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 500. mL. flask with 4.0 atm of methane gas and 1.5 atm of water vapor at 34.0°C. He then raises the temperature, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 0.45 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. Explanation Check

Explanation / Answer

The reaction is CH4(g)+ H2O (g)<--->CO+3H2(g)

Given inital pressures of CH4= 4 atm and that of H2= 1. 5atm

Let P =drop in pressure of H2 to reach equilibirum

At equilibrium, CH4=4-P, H2O= 1.5-P, CO=P and H2=3P

Given 3P= 0.45, P=0.15

So at equilibrium, CH4= 4-0.15=3.85 atm, H2O=1.5-0.15=1.35, CO=0.15 atm and H2=0.45 atm

If P standard for partial pressure of gas

K= [PCO][PH2]3/[PCH4][PH2O]= 0.15*0.45*0.45*0.45/(3.85*1.35)= 0.00263

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