"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrialiy. A chemical engineer studying this reaction filis a 200.mL flask with 3.9atm of carbon monoxide gas and 2.3 atm of water vapor. When the mixture equilibrium she determines that it contains 2.9 atm of carbon monoxide gas, 1.3 atm of water vapor and 1.0 atm of carbon dioxide. The engineer then adds another 2.0 atm of carbon monoxide, and allows the mixture to come to equilibrium again. Calculate the pressure of hydrogen after equilbrium is reached the second time. Round your answer to 2 significant digits. Ammonia will decompose into nitrogen and tydrogen at high temperature. An industrial chemist studying this reaction fills a 5.0L. flask with 4.3 atm of ammonia gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 1.7 atm. Calculate the pressure equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits