Using this balanced equation, I will calculate the 100% mass of Ammonia. I will begin by working out the Atomic Mass of the reactants within the balanced equation. The atomic mass for Nitrogen is 14, however, there are two products of Nitrogen, 14 x 2 = 28 and therefore the total Atomic Mass for Nitrogen equals 28. The Atomic Mass for Hydrogen is 1, in the equation – 3 x 2 = 6 so the total Atomic Mass for Hydrogen is 6.
To conclude this calculation, I will add both the Atomic Mass numbers of Nitrogen and Hydrogen which is 28 + 6 = 34. The 34 is the 100% mass of Ammonia produced.
I will now use my graph to look and calculate the different masses of Ammonia produced at different temperatures using the following equation:
1% of Ammonia = 34/100 = 0.34
Using the equation above, I am now going to take the percentage yield from each different temperature and pressure then multiply the percentage yield by a factor of 0.34 to get the total mass of Ammonia produced.
Table of Results
Table 1 - 350ºc
Table 2 - 400ºc
Table 3 - 450ºc
Table 4 - 500ºc
Table 5 - 550ºc
Analysis
From looking at the chart, I can notice and comment on the trend of the graph. The steepness of the line represents how fast the reaction is and the lines which are shallow show the rate of the reaction decreasing.
On the graph, the shape of the curve gets steeper from the 0 to 200 pressure; the line then continues to curve until the pressure of 400.
Overall, as the pressure increases, the percentage yield of NH3 also increases. As the temperature decreases, the percentage yields increase. I can see this as the curves and points plotted for each temperature get higher on the graph as the temperature decreases. For example, at 350ºc, the percentage yield at 300 is 60% and at 550ºc, the percentage yield at 300 is 16%.
On the graph, I can see that there is an anomalous result for the temperature of 350˚c in the atmosphere of 200 with a percentage yield of 52% for Ammonia.
I can tell that this is an anomalous result as it does not fit on the graph with the other points for 350˚c; it does not appear on the curve and is much higher than the other plotted points for this curve.
As a result of this, I will re-test this to make the results fair, reliable and accurate.
I will now look at each temperature at 400 atmospheres to measure the yield of Ammonia. For the temperature of 350ºc, the percentage yield at the atmosphere of 400 is 65%, for 400ºc, the yield is 50%, for 450ºc the percentage yield is 38%, the yield for 500ºc is 33% and for 550ºc, the percentage yield at 400 atmosphere is 18%. From looking at these results, I can tell that the percentage yield decreases as the temperature increases.
Now I shall compare the percentage yields for two different chosen temperatures from the graph. I have decided to compare percentage yields of 350ºc and 550ºc. For 350ºc, the percentage yield at the pressure of 100 is 32% and the percentage yield for 400 is 65%. Whereas for 550ºc, the percentage yield for the 100 atmosphere is 6% and the yield for the 400 atmosphere is 18%.
Therefore, from looking at my results, I can tell the 350ºc at 400 atmosphere would be best for optimum Ammonium production as the results of percentage yield are higher than the percentage yields for 550ºc.
During the Haber Process, the increasing pressure increases the yield of Ammonia. If we look at a pressure of 200 atmosphere, a fair yield of Ammonia is produced without using costly equipment making the rate of the reaction faster. As the temperature increases, the yield of Ammonia is reduced but the rate of the reaction is also increased.
A chosen temperature of 450ºc is low enough to produce a good yield of Ammonia at a reasonable rate, so I have picked an atmosphere of 200 and a temperature of 450ºc.
The higher the temperature, enough energy is given to the reaction. The reverse reaction for this is known as an endothermic reaction which favours the break down of Ammonia. Whereas if the temperature is low, this favours the Ammonium production as the rate is high, this part of the Haber Process is an exothermic reaction.
When the temperature increases to a certain extent, an endothermic reaction will occur causing the break down of Ammonia.
In the reaction, the heat up of Nitrogen and Hydrogen react to create collisions of particles from the energy. The more collisions that occur, the faster the rate of the reaction will be, the rate is only fast up to the pressure of 200 atmosphere.
The Haber Process is used in industry, the greatest demand of this process is Ammonium production. Ammonia is used as a fertiliser mainly for farming, an advantage of this is that most of the Ammonia is produced at the minimum cost which is favoured from the temperature of 400ºc and pressure 200. The disadvantage of this is that the Ammonia can travel into rivers or streams causing environmental issues such as eutrophication where all wild life i.e. fish can be killed. This is caused from the increase in microbes and the fertiliser being full of nutrients.
The pressure is the economical situation attempting to increase as much pressure as possible. Initially, Haber and Bosch used reaction chambers of Osmium and Uranium catalysts. Currently, Iron Catalyst is used as it is less expensive.
During the Industrial practice, Iron Oxide and Magnetite is used to produce the iron catalyst which is given to the Hydrogen reactants. This decreases the magnetite to metallic Iron and also removes the Oxygen within the process. On the other hand, the catalyst keeps most of its density volume throughout the chemical reaction.
The larger the surface area of the catalyst, the more bulk is maintained and meaning the porous is higher therefore it makes it a more effective catalyst.
Calcium and Aluminium which are other minor components of the catalyst supports the porous and also helps maintain the surface area and the reactivity increases the Potassium which raises the Electron density of the catalyst.
The Ammonia is formed as a gas but cooling the condenser liquefies at the high pressures used and therefore is removed as a liquid. Unreacted Nitrogen and Hydrogen is fed back in to the reaction.
The pressure is the economical situation attempting to increase as much pressure as possible. Initially, Haber and Bosch used reaction chambers of Osmium and Uranium catalysts. Currently, Iron Catalyst is used as it is less expensive.
During the Industrial practice, Iron Oxide and Magnetite is used to produce the iron catalyst which is given to the Hydrogen reactants. This decreases the magnetite to metallic Iron and also removes the Oxygen within the process. On the other hand, the catalyst keeps most of its density volume throughout the chemical reaction.
The larger the surface area of the catalyst, the more bulk is maintained and meaning the porous is higher therefore it makes it a more effective catalyst.
Calcium and Aluminium which are other minor components of the catalyst supports the porous and also helps maintain the surface area and the reactivity increases the Potassium which raises the Electron density of the catalyst.
The Ammonia is formed as a gas but cooling the condenser liquefies at the high pressures used and therefore is removed as a liquid. Unreacted Nitrogen and Hydrogen is fed back in to the reaction.
