Task

__**TASK**__ Open this computer simulation: []
 * Q1. **

**a)** Fill in the table below, by keeping a constant temperature of 350 ° C whilst altering the pressure
 * Pressure (atm) || 100 || 200 || 300 || 400 || 500 || 600 || 700 || 800 || 900 || 1000 ||
 * yield (%) ||  ||   ||   ||   ||   ||   ||   ||   ||   ||   ||

**b)** Fill in the table below keeping a constant pressure of 600atm
 * Temperature  (° C) || 150 || 200 || 250 || 300 || 350 || 400 || 450 || 500 ||
 * yield (%) ||  ||   ||   ||   ||   ||   ||   ||   ||

Label your graphs as “**Pressure (atm) vs. NH3 present (%)**” and “**Temperature (** **° ** **C) vs. NH3 present (%)**”
 * Q2. ** Using the values from the above tables construct 2 graphs to display your results using this graphing tool: [].

**Q3.** Le Chatelier's principle says that, for an exothermic reaction, low temperatures will lead to the production of more of the products (one of which is heat that will warm up the system). Explain whether the graphs support the information that the reaction of nitrogen and hydrogen to give ammonia is exothermic?

**Q4.** Analyse the impact of increased pressure on the whole system involved in the Haber process. (Refer to the information from the graphs as well as Le Chatelier).

**Q5.** Higher temperatures increase the rate of reactions, however the yield of ammonia in the Haber process is reduced at higher temperatures. Explain why, using Le Chatelier's principle.

**Q6.** Recall information about the effect of temperature on rates of reaction. Are there any implications in regards to reaction rate and the choice of temperature for the Haber process? Justify your answer with respect to reaction energy, reaction rate and equilibrium.

**Q7.** Explain that the use of a catalyst will lower the reaction temperature required in the Haber process, and using the internet, find the catalyst that is used during the process. Be sure to supply references.

**Q8.** Using online resources, your text book and class notes, identify what temperature and pressure is the most economical to produce an optimum amount of ammonia?

**Q9.** An example of a HSC question: Production of NH3 is a continuous process. Ammonia, nitrogen and hydrogen are continually removed from the reaction vessel. The gases are cooled when removed and then, after the liquid NH3 is separated, the nitrogen and hydrogen are returned to the reaction. The boiling points of the 3 gases involved in the Haber process are -253 ° C (hydrogen), -33 ° C (ammonia) and -196 ° C (nitrogen). Account for the increased yield of ammonia when the reaction mixture, consisting of all 3 gases, is removed and cooled. Refer to the boiling points given.