Steam reforming of methane ( ) 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 tank with of methane gas and of water vapor, and when the mixture has come to equilibrium measures the amount of carbon monoxide gas to be .Calculate the concentration equilibrium constant for the steam reforming of methane at the final temperature of the mixture. Round your answer to significant digits.

1.5

Explanation:

The reaction between methane and water vapor to produce carbon monoxide and hydrogen gas is

CH4(g) + 2H2O(g) ⇄ CO2(g) + 4H2(g)

The reaction is reversible and achieves the equilibrium when the velocity of the formation of the products and the velocity of the formation of the reagents are the same. In this case, both concentration and pressure remain constant.

The pressure equilibrium constant is the value of the ratio of the multiplication of the partial pressure of the products by the multiplication of the partial pressure of the reagents, each one elevated by the coefficient of the substance.

Thus, doing an equilibrium chart:

CH4(g) + 2H2O(g) ⇄ CO2(g) + 4H2(g)

0.60 atm 2.6 atm 0 0 Initial

-x -2x +x +4x Reacts (stoichiometry is 1:2:1:4)

0.60-x 2.6-2x x 4x Equilibrium

pH2 = 1.4 atm

4x = 1.4

x = 0.35 atm

So, the partial pressures in equilibrium are:

pCH4 = 0.60 - 0.35 = 0.25 atm

pH2O = 2.6 - 2*0.35 = 1.9 atm

pCO2 = 0.35 atm

pH2 = 1.4 atm

Kp = 1.5

frequency, z, and the collision density, z, in carbon dioxide (co2), r 180 pm at 30 °c and 120 kpa