Question

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 degrees Celsius and a pressure of about 200 atm). This process holds 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 controversies followed the Nobel Prize award. For this experiment, 16.55 grams of nitrogen and 10.15 grams of hydrogen gas are allowed to react in the reaction vessel. The ammonia vapor 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. (3 pts) 2. What is the theoretical yield of ammonia (in grams) if 16.55 grams of nitrogen gas and 10.15 grams of hydrogen gas are allowed to react? (9 pts) 3. Based on your theoretical yield, what is the percent yield of ammonia if only 8.33 grams of ammonia are produced? (3 pts) 4. How much heat energy (in kJ) will be absorbed or released if 8.33 grams of ammonia are produced? State whether the energy will be absorbed or released. (4 pts) 5. Ammonia gas reacts with aqueous nitric acid to form aqueous ammonium nitrate, a fertilizer. (a) Write the balanced chemical equation for the reaction, including the physical states. (2 pts)

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 degrees Celsius and a pressure of about 200 atm). This process holds 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 controversies followed the Nobel Prize award.

For this experiment, 16.55 grams of nitrogen and 10.15 grams of hydrogen gas are allowed to react in the reaction vessel. The ammonia vapor 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. (3 pts)

2. What is the theoretical yield of ammonia (in grams) if 16.55 grams of nitrogen gas and 10.15 grams of hydrogen gas are allowed to react? (9 pts)

3. Based on your theoretical yield, what is the percent yield of ammonia if only 8.33 grams of ammonia are produced? (3 pts)

4. How much heat energy (in kJ) will be absorbed or released if 8.33 grams of ammonia are produced? State whether the energy will be absorbed or released.
(4 pts)

5. Ammonia gas reacts with aqueous nitric acid to form aqueous ammonium nitrate, a fertilizer.
(a) Write the balanced chemical equation for the reaction, including the physical states. (2 pts)

Added by Markia S.

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