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 0.60 atm of methane gas and 2.6 atm of water vapor at 47. °C. He then raises the temperature, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 1.4 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

Under what conditions will a gas be most likely to exhibit the ideal gas properties predicted by the ideal gas law? 1)high pressures and high temperature, because particles are forced closer together with higher kinetic energy, so intermolecular forces of attraction are weaker 2)high pressure and low temperature, because particles are forced closer together and moving slower, so the volume of the particles is less significant 3) low pressure and high temperature, because particles are spread farther apart and moving faster, so the intermolecular forces of attraction are weaker 4)low pressure and low temperature, because particles are spread farther apart with lower kinetic energy, so the volume of the particles is less significant