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Human influences and industry

Module by: Free High School Science Texts Project. E-mail the author

Human Influences on the Nitrogen Cycle

Humans have contributed significantly to the nitrogen cycle in a number of ways.

  • Atmospheric pollution is another problem. The main culprits are nitrous oxide (N2O), nitric oxide (NO) and nitrogen dioxide (NO2). Most of these gases result either from emissions from agricultural soils (and particularly artificial fertilisers), or from the combustion of fossil fuels in industry or motor vehicles. The combustion (burning) of nitrogen-bearing fuels such as coal and oil releases this nitrogen as NO2 or NO gases. Both NO2 and NO can combine with water droplets in the atmosphere to form acid rain. Furthermore, both NO and NO2 contribute to the depletion of the ozone layer and some are greenhouse gases. In high concentrations, these gases can contribute towards global warming.
  • Both artificial fertilisation and the planting of nitrogen fixing crops, increase the amount of nitrogen in the soil. In some ways this has positive effects because it increases the fertility of the soil and means that agricultural productivity is high. On the other hand, however, if there is too much nitrogen in the soil, it can run off into nearby water courses such as rivers or can become part of the groundwater supply as we mentioned earlier. Increased nitrogen in rivers and dams can lead to a problem called eutrophication. Eutrophication is the contamination of a water system with excess nurtrients, which stimulates excessive algae growth at the expense of other parts of the ecosystem. This occurs as eutrophication reduces oxygen levels in the water. Sometimes this can cause certain plant species to be favoured over the others and one species may 'take over' the ecosystem, resulting in a decrease in plant diversity. This is called a 'bloom'. Eutrophication also affects water quality. When the plants die and decompose, large amounts of oxygen are used up and this can cause other animals in the water to die.

Case Study : Fertiliser use in South Africa

Refer to the data table below, which shows the average fertiliser use (in kilograms per hectare or kg/ha) over a number of years for South Africa and the world. Then answer the questions that follow:

Table 1
 196519701975198019851990199520002002
SA27.942.257.780.366.654.948.547.161.4
World34.048.963.980.686.790.984.988.291.9
  1. On the same set of axes, draw two line graphs to show how fertiliser use has changed in SA and the world between 1965 and 2002.
  2. Describe the trend you see for...
    1. the world
    2. South Africa
  3. Suggest a reason why the world's fertiliser use has changed in this way over time.
  4. Do you see the same pattern for South Africa?
  5. Try to suggest a reason for the differences you see in the fertiliser use data for South Africa.
  6. One of the problems with increased fertiliser use is that there is a greater chance of nutrient runoff into rivers and dams and therefore a greater danger of eutrophication. In groups of 5-6, discuss the following questions:
    1. What could farmers do to try to reduce the risk of nutrient runoff from fields into water systems? Try to think of at least 3 different strategies that they could use.
    2. Imagine you are going to give a presentation on eutrophication to a group of farmers who know nothing about it. How will you educate them about the dangers? How will you convince them that it is in their interests to change their farming practices? Present your ideas to the class.

The industrial fixation of nitrogen

A number of industrial processes are able to fix nitrogen into different compounds and then convert these compounds into fertilisers. In the descriptions below, you will see how atmospheric nitrogen is fixed to produce ammonia, how ammonia is then reacted with oxygen to form nitric acid and how nitric acid and ammonia are then used to produce the fertiliser, ammonium nitrate.

  • Preparation of ammonia (NH3) The industrial preparation of ammonia is known as the Haber-Bosch process. At a high pressure and a temperature of approximately 50000C, and in the presence of a suitable catalyst (usually iron), nitrogen and hydrogen react according to the following equation: N2 + 3H2 →→ 2NH3 Ammonia is used in the preparation of artficial fertilisers such as (NH4)2SO4 and is also used in cleaning agents and cooling installations.

    Note: Interesting Fact :

    Fritz Haber and Carl Bosch were the two men responsible for developing the Haber-Bosch process. In 1918, Haber was awarded the Nobel Prize in Chemistry for his work. The Haber-Bosch process was a milestone in industrial chemistry because it meant that nitrogenous fertilisers were cheaper and much more easily available. At the time, this was very important in providing food for the growing human population. Haber also played a major role in the development of chemical warfare in World War I. Part of this work included the development of gas masks with absorbent filters. He also led the teams that developed chlorine gas and other deadly gases for use in trench warfare. His wife, Clara Immerwahr, also a chemist, opposed his work on poison gas and committed suicide with his service weapon in their garden. During the 1920s, scientists working at his institute also developed the cyanide gas formulation Zyklon B, which was used as an insecticide and also later, after he left the programme, in the Nazi extermination camps. Haber was Jewish by birth, but converted from Judaism in order to be more accepted in Germany. Despite this, he was forced to leave the country in 1933 because he was Jewish 'by definition' (his mother was Jewish). He died in 1934 at the age of 65. Many members of his extended family died in the Nazi concentration camps, possibly gassed by Zyklon B.
  • Preparation of nitric acid (HNO3) Nitric acid is used to prepare fertilisers and explosives. The industrial preparation of nitric acid is known as the Ostwald process. The Ostwald process involves the conversion of ammonia into nitric acid in various stages: Firstly, ammonia is heated with oxygen in the presence of a platinum catalyst to form nitric oxide and water.
     4NH3(g) + 5O2(g) →→ 4NO(g) + 6H2O(g)
     Secondly, nitric oxide reacts with oxygen to form nitrogen dioxide. This gas is then readily absorbed by the water to produce nitric acid. A portion of nitrogen dioxide is reduced back to nitric oxide.
     2NO(g) + O2(g) →→ 2NO2(g) 3NO2(g) + H2O(l)→→ 2HNO3(aq) + NO(g)
     The NO is recycled and the acid is concentrated to the required strength by a process called distillation.
  • Preparation of ammonium nitrate Ammonium nitrate is used as a fertiliser, as an explosive and also in the preparation of 'laughing gas' which is used as an anaesthetic. Ammonium nitrate is prepared by reacting ammonia with nitric acid:
     NH3 + HNO3 →→ NH4NO3

Debate : Fertiliser use

Divide the class into two groups to debate the following topic:

Increasing the use of artificial fertilisers is the best solution to meet the growing food needs of the world's human population.

One group should take the position of agreeing with the statement, and the other should disagree. In your groups, discuss reasons why you have the opinion that you do, and record some notes of your discussion. Your teacher will then explain to you how to proceed with the debate.

The following presentation shows other ways to represent the nitrogen cycle.

Figure 1

Summary

  • Nitrogen is essential for life on earth, since it forms part of amino acids, proteins and nucleic acids.
  • The atmosphere is composed mostly of nitrogen gas, but the gas is inert, meaning that it is not available to living organisms in its gaseous form.
  • The nitrogen cycle describes how nitrogen and nitrogen-containing compounds are changed into different forms in nature.
  • The nitrogen cycle consists of three major processes: nitrogen fixation, nitrification and denitrification.
  • Nitrogen fixation is the conversion of atmospheric nitrogen into compounds such as ammonia that are more easily used.
  • Nitrogen can be fixed biologically through the actions of bacteria, industrially through the Haber-Bosch process or by lightning.
  • Nitrification converts ammonia into nitrites and nitrates, which can be easily assimilated by plants.
  • Denitrification converts nitrites and nitrates back into gaseous nitrogen to complete the nitrogen cycle.
  • Humans have had a number of impacts on the nitrogen cycle. The production of artificial fertilisers for example, means that there is a greater chance of runoff into water systems. In some cases, eutrophication may occur.
  • Eutrophication is the contamination of a water system with excess nurtrients, which stimulates excessive algae growth at the expense of other parts of the ecosystem. This occurs as eutrophication reduces oxygen levels in the water.
  • Many nitrogen gases such as NO, N2O and NO2 are released by agricultural soils and artificial fertilisers. These gases may combine with water vapour in the atmosphere and result in acid rain. Some of these gases are also greenhouse gases and may contribute towards global warming.
  • A number of industrial processes are used to produce articifical fertilisers.
  • The Haber-Bosch process converts atmsopheric nitrogen into ammonia.
  • The Ostwald process reacts ammonia with oxygen to produce nitric acid, which is used in the preparation of fertilisers and explosives.
  • If ammonia and nitric acid react, the product is ammonium nitrate, which is used as a fertiliser and as an explosive.

Summary Exercise

  1. Look at the diagram and the descriptions of the nitrogen cycle earlier in the chapter:
    1. Would you describe the changes that take place in the nitrogen cycle as chemical or physical changes? Explain your answer.
    2. Are the changes that take place in the water cycle physical or chemical changes? Explain your answer.
    Click here for the solution
  2. Explain what is meant by each of the following terms:
    1. nitrogen fixing
    2. fertiliser
    3. eutrophication
    Click here for the solution
  3. Explain why the fixing of atmospheric nitrogen is so important for the survival of life on earth. Click here for the solution
  4. Refer to the diagram below and then answer the questions that follow:
    Figure 2
    Figure 2 (CG10C7_001.png)
    1. Explain the role of decomposers in the nitrogen cycle.
    2. If the process taking place at (3) is nitrification, then label the processes at (1) and (5).
    3. Identify the nitrogen products at (2) and (4).
    4. On the diagram, indicate the type of bacteria that are involved in each stage of the nitrogen cycle.
    5. In industry, what process is used to produce the compound at 2?
    6. Does the diagram above show a 'cycle'? Explain your answer.
    Click here for the solution
  5. NO and NO2 are both nitrogen compounds:
    1. Explain how each of these compounds is formed?
    2. What effect does each of these compounds have in the environment?
    Click here for the solution
  6. There are a number of arguments both 'for' and 'against' the use of artificial fertilisers. Draw a table to summarise the advantages and disadvantages of their use. Click here for the solution

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