A research team is testing the combustion reaction of methane with oxygen. The balanced chemical equation is CH4 + 2O2 → CO2 + 2H2O. The team is using an 8.20-liter closed container at 30.0°C. The partial pressure of methane is 130.0 kilopascals, and the partial pressure of oxygen is 142 kilopascals. What is the limiting reactant and the mass of carbon dioxide produced in the combustion reaction?

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.