3) A rigid 11.7 L sealed vessel containing 3.3 mol of O2(e), 1.6 mol of CH4(g), and 2.3
mol of He has an internal temperature of 78°C.
a. Calculate the partial pressure of each gas.
b. W hat is the total pressure in the vessel?
c. Find the mole fraction of each gas in the vessel.
d. A lab technician ignites the mixture in the flask and the following reaction
occurs: CH4(g) +2 02(g)→ CO2(g) + 2 H2O(g). Find the mole fraction of
each gas in the mixture after the reaction.
(Hint: Use an ICE chart. There is a limiting reactant.)

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 1.5 l flask with 3.5 atm of methane gas and 1.3 atm of water vapor at 43.0°c. he then raises the temperature, and when the mixture has come to equilibrium measures the partial pressure of carbon monoxide gas to be 1 .0 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.