Write a balanced thermochemical equation with phase labels for the Haber process with the heat energy as part of the equation.

While the majority component of air is nitrogen (N₂), the gas is very unreactive because of its stability due to the triple bonds that hold the nitrogen atoms together.  Nitrogen gas is, therefore, relatively unavailable for chemical reactions.  One of the few ways to “fix” nitrogen, making a nitrogen compound from the elemental nitrogen in the atmosphere, is the Haber process (aka Haber-Bosch process).  In this reaction, nitrogen gas combines with hydrogen gas to yield ammonia.  The enthalpy (ΔH) of this reaction is 92.22 kJ.

This process was discovered by the German chemist Fritz Haber in the early twentieth century.  Through extensive experimentation, Haber found the conditions that would produce adequate yields (at a temperature of about 500 ^oC and a pressure of about 200 atm).  This process holds a significant importance today because of its application in the industrial production of ammonia-based fertilizer.  In 1918, Haber received the Nobel Prize in Chemistry for his work.  However, a lot of controversy followed the Nobel Prize award.

For this experiment, 16.55 grams of nitrogen gas and 10.15 grams of hydrogen gas are allowed to react in the reaction vessel.  The ammonia vapor that is produced is then condensed, liquefied, and collected into a collection vessel.

1. Write a balanced thermochemical equation with phase labels for the Haber process with the heat energy as part of the equation.