In the important industrial process for producing ammonia (the haber process), the overall reaction is:
n2(g) + 3h2(g) 2nh3(g) + 100.4 kj
a yield of nh3 of approximately 98% can be obtained at 200°c and 1,000 atmospheres of pressure.
how many grams of ny must react to form 1.7 grams of ammonia, nh3?
0.052 g
1.49
0.00589
2.8 g

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.