• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

Research into the production of Nitrate Fertillisers.

Extracts from this document...


Part 1: stimulus material: Research and collecting secondary data. Advantages of Ammonium Nitrate Fertilizer Ammonium (NH4+) and nitrate (NO3-) are the two forms in which plants can directly utilize nitrogen from the soil. Upon application of ammonium nitrate fertilizer, it easily dissociates into these two forms. When urea-based fertilizers are used, conversion of urea to ammonium occurs for a period of one day to one week and some amount of nitrogen is lost to the atmosphere in the process. Thus, the immediate availability of nitrate ions makes ammonium nitrate preferable over urea-based ones. Moreover, ammonium nitrate is a stable fertilizer and is not subject to losses due to volatilization. Ammonium nitrate, is widely used in mining and construction industries, in the form of dry blasting agents. Being available in the crystalline dry forms, it is easy to handle and load. Moreover, they are safe and cheap as compared to other blasting agents. Disadvantages of ammonium Nitrate Fertilizer As I said earlier, ammonium nitrate is a strong and explosive agent. ...read more.


Ammonium nitrate is commonly mixed with other fertilizers, but these mixtures cannot be stored for long periods because of a tendency to absorb moisture from the air. The very high solubility of ammonium nitrate makes it well suited for making solutions for fertigation or foliar sprays. Ammonium Sulfate Ammonium sulfate [(NH4)2 SO4] was one of the first and most widely used nitrogen (N) fertilizers for crop production. It is now less commonly used, but especially valuable where both N and sulfur (S) are required. Its high solubility provides versatility for a number of agricultural applications. Chemical Properties of Ammonium sulfate Chemical formula: (NH4)2SO4 N content: 21% S content: 24% Water solubility 750 g/L Solution pH 5 to 6 Agricultural use of ammonium sulphate Ammonium sulfate is used primarily where there is a need for supplemental N and S to meet the nutritional requirement of growing plants. used in flooded soils for rice production, where nitrate-based fertilizers are a poor choice due to denitrification losses. ...read more.


Ammonium sulphate is formed by reacting ammonia with sulphuric acid. Phosphate fertilisers The production of phosphate fertilisers also involves a number of processes. The first is the production of sulphuric acid through the contact process. Sulphuric acid is then used in a reaction that produces phosphoric acid. Phosphoric acid can then be reacted with phosphate rock to produce triple superphosphates. The production of sulfuric acid Sulfuric acid is produced from sulphur, oxygen and water through the contact process. In the first step, sulphur is burned to produce sulphur dioxide. This is then oxidised to sulphur trioxide using oxygen in the presence of a vanadium(V) oxide catalyst. Finally the sulphur trioxide is treated with water to produce 98-99% sulfuric acid. Nutrients are very important for life to exist. An essential nutrient is any chemical element that is needed for a plant to be able to grow from a seed and complete its life cycle. The same is true for animals. A macronutrient is one that is required in large quantities by the plant or animal, while a micronutrient is one that only needs to be present in small amounts for a plant or an animal to function properly. ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our International Baccalaureate Chemistry section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related International Baccalaureate Chemistry essays

  1. Analysis of the Nitrogen Content of Lawn Fertiliser

    6. Repeat Step 5 with each of the other two conical flasks. 7. Rinse and fill a burette with standard HCl. Record the concentration of the acid and the initial burette reading. 8. Add two to three drops of methyl red indicator to each conical flask containing the fertilizer mixture, and titrate.

  2. Using Solubility Rules to Indentify Unknown Solutions

    Record the result of each test by using a key eg. NR for No Reaction, and ppt for precipitate. Record all results in a table. Also record any colour changes and comment on the consistency of the precipitation (ie what does it look like?

  1. Free essay

    Energy content Cal/g

    Final Mass of food (+/- .005g) Time ( Seconds) Temperature (+/- .5 �C) Water (+/- .5ml) One 0.81 0.26 0 24 50 15 24 30 25 45 26 60 28 75 29 Two 0.81 0.25 0 23 50 15 23 30 24 45 24 60 25 75 26 Three 0.82

  2. Chemical monitoring and management - composition of the atmosphere and the problems of pollution.

    hence in 1987 the Montreal protocol was signed by nations to alleviate the use of CFCs. The protocol has been extremely affective and all developed countries have ceased used of CFCs, although 3rd world countries still use them. New alternative chemicals have been introduced such as the hydrochlorofluorocarbons (HCFCs)

  1. Examining the Solubility of Substances in Double Replacement Reactions (Final)

    AgBr(s) AgNO3 - CuSO4 : Overall equation: 2AgNO3(aq) + CuSO4(aq) Ag2SO4(s) + Cu(NO3)2(aq) Net Ionic Equation: 2Ag+(aq) + SO42-(aq) Ag2SO4(s) A precipitate has been produced although the table points out that no observation has been made. AgNO3 - NaI : Overall equation: AgNO3(aq) + NaI(aq) AgI(s) + NaNO3(aq)

  2. Enzyme In Industry

    Conclusion: Above as seen from the results there's a clear relation between the rate at which the reaction takes place and the rate of change of that rate. This Is all due to the fact that the more collisions between the acid molecules and the magnesium molecules there are, the

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work