The Uses of Sulphuric Acid in Daily life Manufacture fertiliser Manufacture detergents Manufacture pesticides Manufacture synthetic fibres Manufacture paint pigments As the electrolyte in lead-acid accumulators To remove metal oxides from metal surface SULPHURIC ACID 1
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The Uses of Sulphuric Acid in Daily life
Manufacture fertiliser
Manufacture detergents
Manufacture pesticides
Manufacture synthetic fibres
Manufacture paint pigments
As the electrolyte in lead-acid accumulators
To remove metal oxides from metal surface
SULPHURIC ACID
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Environmental Pollution by Sulphur Dioxide
Pollution of Sulphur Dioxide
Burning of fossil fuels
Fossil fuels such as petroleum.It contain sulphur.Sulphur dioxide is produced when fossil fuels are burned
Affects the respiratory system
Sulphur is a poisonous and acidic gas.It causes coughing, chest pains, shortness of breath, lung diseases and bronchitis
Burning of sulphur in industrial area
The contact process and the burning of coals or fuels produce high sulphur dioxide content
Affect of acid rain
Sulphur dioxide gas dissolve in atmospheric water to produce sulphurous acid, H2SO3 and sulphuric acid,H2SO4. These acids causes acid rain.
Acid rains
corrodes
concrete building
and metal
structures
Acid rain increase the acidity of
soil, unsuitable for growth and
destroys the roots of plants.
Acid rain reacts with minerals in the soil to produce salts which are leashed out of the top soil; essential nutrition for plants growth are depleted (plants die of malnutrition and diseases)
Acid rain increase the acidity
of water in lake and rivers,
causes aquatic organisms die
and disturbs the ecosystem
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The
Indu
stria
l Pro
cess
in M
anuf
actu
re o
f Sul
phur
ic A
cid
Stag
e 1
Stag
e 2
Stag
e 3
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Stage 1• Burning of sulphur in dry air in the furnace
• Burning of metal sulphides such as zinc sulphide also produces sulphur dioxide.
• The sulphur dioxide is mixed with excess air. The mixture is then died and purified to remove impurities such as arsenic compounds.
• Arsenic compounds found in sulphur will poison the catalyst in the converter , make the catalyst ineffective
Production of sulphur dioxide gas, SO2
S(s) + O2(g) SO2(g)
• Mixture of sulphur dioxide and excess dry oxygen is passed through a converter.
• Sulphur dioxide is oxidised to sulphur trioxide.• 98%conversion from sulphur dioxide to sulphur trioxide is
Stage 2 Conversion of sulphur dioxide to sulphur trioxide, SO3
Stage 3 • In the absorber, sulphur trioxide is dissolve in concentrated sulphuric acid to produce oleum , H2S2O7 a viscous liquid.
• Oleum is then diluted with equal volume of water to produce concentrated H2SO4 (98%)
Production of sulphuric acid
Flow Chart of Contact Process
Sulphur Sulphur Dioxide, SO2
Oleum, H2S2O7
Sulphur trioxide , SO3
Sulphuric acid , H2SO4
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AMMONIA AND ITS SALT
THE USES OF AMMONIA IN INDUSTRY
Nitric acid
Detergents
Prevent coagulation of latex
Paint and colouring
Synthetic fabric
Explosive (TNT)
Synthetic fertiliser
Cooling agent
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The manufacture of nitrogenous fertiliser
Ammonia reacts with sulphuric acid through neutralisation to produce ammonium sulphate
Ammonium sulphate
2NH3(aq) + H2SO4(aq) (NH4)2SO4(aq)
Ammonia reacts with nitric acid through neutralisation to produce ammonium nitrate
NH3(aq) + HNO3(aq) NH4 NO3(aq)
Ammonium nitrate
Ammonia reacts with carbon dioxide at temperature of 200°C and pressure of 200 atmosphere to produce urea
urea
2NH3(g) + CO2(g) CO(NH2)2(s)+H2O(l)
Ostwald process • In the Ostwald process, ammonia is concerted into nitric acid by three stages
Ammonia is oxidised to nitrogen monoxide gas in the presence of platinum as catalyst
4NH3(g) +5O2(g) 4NO(g) + 6H2O(g)
Stage 1
Nitrogen monoxide is further oxidised to nitrogen dioxide
2NO(g) + O2(g) 2NO2(g)
Stage 2
Nitrogen dioxide is dissolve in water to produce nitric acid
2NO(g) + H2O(l) HNO3(aq) + HNO2(aq)
Stage 3
The properties of ammoniaVery soluble
in water
Change red litmus paper blue
Colourless and pungent gas
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The Industrial Process in the Manufacture of Ammonia
The nitrogen and hydrogen gases are combined
The gases are compressed at 200 atmosphere, 450°C
The gases pass through the converter. Iron is used as a catalyst
The Gases are cooled down until the ammonia condenses
Ammonium fertilisers The ammonium stored as a liquid under pressure. The excess hydrogen and nitrogen gases are recycled to continue the reaction• Nitrogen is absorbed by plants in the form of
soluble nitrates, NO3- to produce protein • Ammonium fertilisers are used to replace elements
in soil used up by plants.• Ammonium ions, NH4
+ 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:
Percentage of nitrogen by weight
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The physical properties of pure metal
Ductile • Ductile is the
ability to be stretched
Malleable• Malleable is
the ability of a metal to be shape
High melting and boiling point• The strong force of
attraction between metal atoms requires high energy to overcome it. Hence, metal have high melting points.
High density• In solid state, the atoms
in pure metal are orderly arrange and closely packed, causes pure metal to have high density
Good conductors
Alloys
Meaning and purpose of making alloys
Aim of making alloys
• Pure metal such iron and tin are easily corrode in polluted , damp or acidic air
• Alloying can prevent metals from corrosion due to the formation of oxide layer on the surface of the metal
To prevent corrosion
• Adding the little carbon to iron metal produces steel which is very hard alloy of iron
• Adding magnesium to aluminium metal produces an alloy called Magnalium
• Adding tin copper metal produces bronze. Bronze is an alloy harder than tin and copper
• Pure metal can rust and tarnish easily because of the formation of metal oxides
• Alloying can maintain the lustre on the surface of metal