The production of ammonia (NH3) is achieved industrially via the Haber-Bosch process, which consumes 1-2% of the world's energy supply each year. The reaction occurring is shown below: N2(g) + 3 H2(g) → 2 NH3(g) Suppose that 6.8 L of NH3(g) is collected at 513 K, with a total pressure of 95.2 atm by this process. The partial pressures of N2(g) and H2(g) in the same vessel are 23.28 atm and 50.60 atm, respectively. Answer all four parts of this question. a) What is the partial pressure (in atm) of ammonia gas in the sample? b) What is the mol fraction of ammonia gas? c) How many moles of ammonia gas are produced? d) How many liters of hydrogen gas must have reacted to produce this quantity of ammonia gas if the initial reaction vessel had a hydrogen pressure of 75 atm at 585 K?

15. A student collected 18.45 ml of H2 over water at 24°C. The pressure of the water vapor at this temperature is 22.81 torr. The barometric pressure was 746 torr. How many grams of zinc had to react with HCI(aq) to produce the hydrogen that was collected?

A mixture of xenon and argon gases, in a 9.94 L flask at 74 °C, contains 23.9 grams of xenon and 5.38 grams of argon. The partial pressure of argon in the flask is atm and the total pressure in the flask is atm.

Xenon hexafluoride was one of the first noble gas compounds synthesized. The solid reacts rapidly with the silicon dioxide in glass or quartz containers to form liquid XeOF and gaseous silicon tetrafluoride. What is the pressure in a 1.00-L container at 25 °C after 8.90 g of xenon hexafluoride reacts? (Assume that silicon tetrafluoride is the only gas present and that it occupies the entire volume.) Be sure your answer has the correct number of significant figures. 4 Note: Reference the Fundamental constants table for additional information. atm ☐ x10 X