The document discusses the various uses of ammonia in industry and its production. It describes how ammonia is used to produce nitric acid, detergents, synthetic fabrics, explosives, and as a refrigerant. It also outlines the manufacturing processes for nitrogenous fertilizers like ammonium sulfate, ammonium nitrate, and urea which are produced through neutralization reactions of ammonia with acids. The Ostwald process for producing nitric acid from ammonia is also summarized.

1. GROUP MEMBER:
AISHWARYA CHANDRAN
HANIS KHALIESAH BT MOHD FOUZI
FATIN NABILAH BT RIZA

2. USES OF AMMONIA IN
INDUSTRY
 NITRIC ACID
As a raw material for the manufacture of nitric acid in the Ostwald process.
 DETERGENTS
When ammonia reacts with oil from the plants,detergent is produced.
 PREVENT COAGULATION OF LATEX
Latex can be stored for longer period of time before exporting to other
countries.
 PAINT AND COLOURING
Reaction of nitric acid and organic compound can produce various types of
colouring.
 SYNTHETIC FABRIC
Ammonia is used to synthesis the synthetic fabric such as nylon.
 EXPLOSIVE(TNT)
Reaction of nitric acid and toluena produces explosive material.
 COOLING AGENT
Ammonia is used as cooling agent in the refrigerator because ammonia is
highly compressible,high heat capacity,low boiling point and very volatile.
 Dry cells
Ammonia is used to produce ammonium chloride for an electrolyte in dry
cell

3. THE MANUFACTURE OF
NITROGENOUS FERTILISERS
 Ammonium sulphate
Ammonia reacts with sulphuric acid through
neutralisation to produce ammonium sulphate.
2NH4(aq) +H2SO4(aq) (NH4)2SO4(aq)
 Ammonium nitrate
Ammonia reacts with nitric acid through neutralisation to
produce ammonium nitrate.
NH3(aq)+HNO3(aq) NH4NO3(aq)
 Urea
Ammonia reacts with carbon dioxide at temperature of 200
C a pressure of 200 atmosphere to produce urea
2NH3(aq)+ CO2(g) CO(NH2)2(S)+H2O(L)

4. Ostwald process
 Ammonia is converted into nitric acid by following
this steps:
 Stage 1
Ammonia is oxidised to nitrogen monoxide gas in the
presence of platinum as the catalyst.
4NH3 + 5O2 platinum 4NO + 6H2O
• Stage 2
Nitrogen monoxide is further oxidised to nitrogen
dioxide.
2NO + O2 2NO2
• Stage 3
Nitrogen dioxide is dissolved in water to produce nitric
acid.
4NO2 + O2 + 2H2O 4HNO3

5. The Properties Of Ammonia
o Colourless and pungent gas
It is less dense than air.
o Alkaline gas
Ammonia turns the damp red litmus paper to blue.
o Very soluble in water.
An inverted filter funnel is used to
prevent the sucking back of water.
o To test for ammonia gas
Ammonia gas reacts with hydrogen chloride gas to
to form white fumes of ammonium chloride.
o Neutralisation
Ammonia is a weak alkali which reacts with dilute acids in neutralisation to
produce salts.
o Does not burn in air
Ammonia gas burn in oxygen to produce nitrogen monoxide gas.
o Reacts with aqueous metal ions
Aqueous solutions of ammonia react with metal ions(except Na+ , K+ and
Ca2+) to produce precipitate of metal hydroxides.

6. The Industrial Process in the
Manufacture of Ammonia
 Massive production of ammonia n an industrial sector
is known as Haber process.
 Nitrogen gas used in Haber process is obtained from
the fractional distillation of liquid air.
 Hydrogen gas can be obtained by 2 methods:
 Reaction between steam and heated coke(carbon).
H2O+C CO+H2 mixture is known as
water gas.
 Reaction between steam nd natural gas consist
mainly of methane,CH4.
2H2O+CH4 CO2+4H2

8. Ammonium Fertilisers
 Nitrogen is absorbed by plants in the form of soluble
nitrates to produce protein.
 Ammonium fertilisers are chemical fertilisers that are
used to replaced elements in soil used up by plants.
 Ammonium ions, can be converted into
nitrate ions by bacteria living in the soil.
 The fertiliser with higher percentage of nitrogen is
more effective and this can be determined as below:
Mass of nitrogen
= —————————————— ×100%
Relative molecular mass of fertiliser

9. Example:
 Calculate the percentage by mass of nitrogen in
ammonium sulphate,(NH4)2SO4.[Relative atomic
mass:N,14;H,1;S,32;O,16]
Answer:
Relative molecular mass of(NH4)2SO4
=2 [14 + 4 (1) ] + 32 + 4 (16) =132
1 mol (NH4)2SO4 consistsof 2 mol atoms of nitrogen.
Percentage of nitrogen in 1 mol of (NH4)2SO4
= 2 (4) × 100 % = 21.2 %
132