15102759 chemistry-folio-chapter-9-spm

Hafiz Akmal 1
CHEMISTRY FOLIO chapter 9: Manufacture Substances in industry

SULPHURIC ACID

In the pure, concentrated
sulphuric acid is a diprotic form, sulphuric acid is an
(dibasic) mineral acid oily, colourless liquid
which does not volatise. which is dense and
viscous.

It has high boiling
point, that is 270 ˚C

Hafiz Akmal 2

USES OF SULPHURIC ACID

18%
1%
38% making fertiliser

12% paints

chemicals

detergents
18%
13% removing dust from steel

other uses

Figure 1:- Uses of Sulphuric Acid, H2SO4

Hafiz Akmal 3

2H2SO4 (l) + Ca3(PO4)2 (s) Ca(H2PO4)2 (l) + 2CaSO4 (s)

superphosphate
fertilisers :-
- it is manufactured
from the reaction
between sulphuric
acid and calcium
phosphate.

sulphuric
acid:
making
fertiliser

Ammonia Sulphate
Potassium Sulphate:-
fertiliser:-
- It is manufactured by
- It is manufactured
the neutralisation of
by the neutralisation
sulphuric acid
of sulphuric acid and
potassium hydoxide
ammonia

2KOH(aq) + H2SO4(aq) K2SO4(aq) + 2H2O (l) 2NH3(aq) + H2SO4(aq) (NH4)2SO4(aq)

Hafiz Akmal 4

MANUFACTURE OF SULPHURIC ACID

The manufacture of sulphuric acid in industry is through the
contact process.
The raw materials used to manufacture the acid are sulphur, air
and water.
The acid is produced in 3 stages:-

Stage 1: The production of sulphur dioxide

Stage 2: Formation of sulphur trioxide

Stage 3: Formation of sulphuric acid

Hafiz Akmal 5

STAGE 1:
THE PRODUCTION OF SULPHUR DIOXIDE

a) This can be obtained through two methods:-
a) Heating liquid sulphur with hot air in a furnace.
S (s) + O2 (g) SO2 (g)
b) Heating sulphides in air, for example:
4FeS2 (s) + 11O2 (g) 2Fe2O3 (s) + 8SO2 (g)
SO2 is a side-product in the extraction of the metal, iron.
[Fe2O3 is reduced to iron with coke]
Zinc pyrites can also be heated in air as follows:
2ZnO (s) + 3O2 (g) 2SO2 (g) + 2ZnO (s)

Hafiz Akmal 6

STAGE 2:
FORMATION OF SULPHUR TRIOXIDE

a) Pure, dry sulphur dioxide is mixed with dry oxygen in excess and
passed over vanadium(V) oxide, V2O5 as catalyst at a temperature
of 450˚C - 550˚C and a pressure of 1 atmosphere. The conditions
ensure the maximum production of sulphur trioxide:
2SO2 (g) + O2 (g) 2SO3 (g)
b) The reaction takes place in a heat converter.
c) Excess air is used to ensure higher percentage of SO3 produced.

Hafiz Akmal 7

STAGE 3:
FORMATION OF SULPHURIC ACID

a) The sulphur trioxide is dissolved in concentrated sulphuric acid to
form a product called oleum, H2S2O7. This is carried out until the
concentrated sulphuric acid has reached a concentration of
99.5%.
SO3 (g) + H2SO4 (aq) H2S2O7 (l)
b) The product, oleum will not show any property of an acid. This is
because, oleum will ‘not ionise’ without the presence of water.
c) Water is then added to the oleum to produce concentrated
sulphuric acid.
H2S2O7 (l) + H2O (l) 2H2SO4 (l)
d) The reaction in (a) and (b) is equivalent to dissolving sulphur
trioxide in water.
SO3 (g) + H2O (l) H2SO4 (aq)
e) However, this reaction is not carried out in industry. This is
because the reaction is too vigorous.
f) It produces a large cloud of sulphuric acid mist. This mist is
corrosive and pollutes the air.

Hafiz Akmal 8

CONTACT PROCESS:

Water

Concentrated H2SO4

O2 , V2O5, 450˚C, 1 atm
concentated
Oleum sulphuric
H2S2O7 acid, H2SO4
Burnt in air
Sulphur
trioxide SO3
Sulphur
dioxide SO2

Sulphur

Figure 2:- Flow chart of Contact Process

Hafiz Akmal 9

The industrial process in the Manufactured of Sulphuric Acid

Hafiz Akmal 10

USES OF AMMONIA IN INDUSTRY:
Examples are ammonium sulphate, ammonium nitrate and urea.
The first two are prepare through neuralisation but urea is
produced by the reaction of ammonia with carbon dioxide. The
To reaction involved are as the following:
manufacture
nitrogenous
a) 2NH3 (g) + H2SO4 (aq) (NH4)2SO4 (s) ammonium sulphate
fertilisers b) NH3 (g) + HNO3 (aq) NH4NO3 (aq) ammonium nitrate
c) 2NH3 (g) + CO2 (g) (NH2)2CO (s) + H2O (l) urea

Having a low melting point,
liquefied ammonia makes a good
As a cooling cooling agent in refrigerators and
agent
air conditioners.

It neutralizes the organic acids formed
To prevent the
by microorganisms in latex, thereby
coagulation of preventing coagulation and preserving
latex in the the latex in liquid form.
rubber industry

Ammonia is converted to nitric acid in the Ostwald process:

1) ammonia is first oxidised to nitrogen monoxide, NO, by
oxygen in the presence of platinum as catalyst at 900˚C.
To manufacture 4NH3 (g) + 5O2 (g) Pt/900˚C 4NO (aq) + 6H2O (l)
nitric acid in 2) nitrogen monoxide is further oxidised to nitrogen
industry
dioxide.
2NO (g) + O2 (g) 2NO2 (g)
3) Nitrogen dioxide and oxygen are dissolved in water to
produced nitric acid.
4NO2 (g) + O2 (g) + H2O (l) 4HNO3 (aq)

a) Nitric acid is manufactured from ammonia before
To manufacture being used to make explosive like trinitrotoluene
explosive (TNT).
b) Nitric acid, in this case, is reacted with organic
substances like toluene.

Hafiz Akmal 11

EXPERIMENT TO INVESTIGATE THE
PROPERTIES OF AMMONIA

Aim:-
To investigate the properties of ammonia

Material:-
0.1 mol dm ammonia solution, 0.1 mol dm sodium hydroxide
solution, ammonia chloride, calcium hydroxide, concentrated
hydrochloric acid, soda lime, distilled water, red litmus paper, Ph
paper.

Apparatus:-
Test tubes, beaker, U-tube, Bunsen burner, glass rod, delivery
tube, stoppers.

Procedure:-
a) Preparation of ammonia gas:
1. Some ammonium chloride is mixed with some calcium
hydroxide.
2. The apparatus as shown in Figure 3 is set up

Hafiz Akmal 12

3. The mixture is heated
4. The ammonia gas produced is collected in a few test tubes.
The test tubes containing ammonia gas must be closed with
stoppers.

b) Alkalinity of ammonia:
1. 5.0 cm of 1 mol ammonia solution and 5 cm of 0.1 mol dm
sodium hydroxide solution are poured into two separate test
tubes.
2. A piece of pH paper is dipped into the solution in each test
tube.
3. The pH values of both solution are recorded.

c) Colour, physical state, smell and solubility of ammonia:
1. The colour and physical state of ammonia are observed.
2. The stopper of a test tube containing ammonia gas is
removed and the smell of the gas is identified.
3. A test tube containing ammonia gas is inverted into a beaker
of water.
4. All observation are recorded.

Hafiz Akmal 13

d) Density of ammonia:
1. A test tube containing ammonia gas is held upright and
another test rube containing ammonia gas is held upside
down.
2. The stopper of the two test tubes are removed.
3. After 20 seconds, a piece of moist red litmus paper is put at
the mouth of each test tube as shown in figure 5.
4. The colour of the red litmus paper is recorded.

e) Chemical property of ammonia:
1. One end of a glass rod is dipped into concentrated
hydrochloric acid.
2. The glass rod is then put on top of a test tube of ammonia
gas.
3. Any change taking place is observed.

Hafiz Akmal 14

Observation :-

Section Observation Inference
pH of ammonia
ammonia is weak
solution is 10
alkali
b) pH of sodium
sodium hydroxide
hydroxide solution
is a strong alkali
is 14
colourless gas ammonia is a
pungent smell colourless gas with
c) water rushed up a pungent smell
and fills up the ammonia is very
whole test tube soluble in water
moist red litmus
paper on top of the
upright test tube Ammonia gas has
does not change escaped from the
d) colour. upright test tube
Moist red litmus and thus is slightly
paper under the less dense than air
inverted test tube
turns blue
Ammonia react
with hydrogen
Dense white fumes
e) are formed
chloride gas to
form ammonium
chloride

Hafiz Akmal 15

Discussion:-
Ammonia is a weak alkali and has a pH of 10
Ammonia is a colourless gas with a pungent smell
Ammonia is very soluble in water, ionize partially in water to form
ammonium ions and hydroxide
NH3 (g) + H2O (l) = NH4+ (aq) + OH- (aq)
Ammonia is slightly less dense than air
Ammonia react with hydrogen chloride gas to form ammonium
chloride
NH3 (g) + HCl (g) = NH4Cl (s)

Conclusion:-
Ammonia is an alkaline, colourless gas with a pungent smell. It is
very soluble in water and is less dense in than air. It react with
hydrogen chloride gas to form dense white fumes of ammonium
chloride

Hafiz Akmal 16

HABER PROCESS

Hafiz Akmal 17

The manufacture of ammonia through the Haber Process

Hafiz Akmal 18

PREPARATION OF AMMONIA FERTILISER

Aim:-
To prepare ammonium sulphate.

Material:-
1 mol dm-2 sulphuric acid, 2 mol dm-3 ammonia solution, methyl
orange, filter paper

Apparatus:-
25.0 cm pipette, burette, conical flask, white tile, retort stand and
clamp, beaker, glass rod, evaporating dish, filter funnel, Bunsen
burner, tripod stand, wire gauze.

Procedure:-
a) Determining the volume of sulphuric acid that will neutralize 25.0
cm of ammonia solution:-
1. 25.0 cm of 2 mol dm-3 ammonia solution is transferred by a
pipette to a clean conical flask.
2. Three drops of methyl orange indicator are added to the
alkali. The solution turns yellow.

Hafiz Akmal 19

3. A clean burette is filled with 1 mol dm-2 sulphuric acid and
clamped to a retort stand. The initial burette reading is
recorded.
4. The conical flask with its content is placed on a white tile
below the burette as shown in figure 6 below.

5. The sulphuric acid is added slowly into the conical flask. The
conical flask is swirled gently throughout the titration.
6. The addition of sulphuric acid is stopped when the indicator
changes from yellow to orange. The final burette reading is
recorded.
7. The volume of acid needed to completely neutralize the 25.0
cm of 2 mol dm-3 ammonia solution is calculated. Let this
volume V cm.

Hafiz Akmal 20

b) Preparation ammonium sulphate salt:-

1. 25.0 cm of 2 mol dm-3 ammonia solution is pipetted into a
clean conical flask. No indicator is added.
2. V cm of 1 mol sulphuric acid is added from the burette to the
ammonia solution.
3. The mixture in the conical flask is transferred to an
evaporating dish and heated until a saturated solution is
formed.
4. The hot, saturated salt solution is left to cool for
crystallization to occur.
5. The crystal of ammonium sulphate formed are filtered,
ashed and dried between sheets of filter paper.

Observation:-
A colourless solution is formed when sulphuric acid is added to
ammonia solution.
The crystal obtained are white in colour

Hafiz Akmal 21

Discussion:-
The equation for the reaction is:
H2SO4 (aq) + 2NH4OH (aq) (NH4)2SO4 (aq) + 2H2O (l)
Methyl orange is an acid-base indicator used to determine the
end point of the titration.
The first titration is carried out to determine the exact volume of
sulphuric acid required to completely neutralize the 25.0 cm of
ammonia solution.
The salt solution in the first titration is discarded because it is
contaminated by methyl orange.
The ammonium sulphate solution should not be heated until
dryness because ammonium sulphate decomposes when it is
overheated.
The weight of ammonium sulphate obtained from the activity is
always less than the theorical value. This is because some of the
salt is not fully crystallized out and still remains in the solution.
Other ammonium salt such as ammonium nitrate can be prepared
from the reaction between nitric acid and ammonium solution.

Conclusion:-
Ammonium sulphate and other ammonium fertilizers can be
prepared by neutralizing ammonia solution with the respective
acids.

Hafiz Akmal 22

THE PHYSICAL PROPERTIES OF PURE
METAL

Hafiz Akmal 23

PROPERTIES OF AMMONIA

Ammonia turns
the damp red
litmus paper
blue.
The gas is less
dense than air
+ -
NH3 + H2O NH4 OH

alkaline
An inverted filter funnel is used gas, colurless
and pungent
to prevent sucking back of water gas Aqueous solutions of ammonia
react with metal ions (except
Na+, K+, and Ca2+) to produce
precipitate of metal hydroxide

Ammonia is weak alkali which
reacts with dilute acids in
neutralization to produce salt.
Ammonia gas burns in oxygen to 2NH3 + H2SO4 (NH4)2SO4
produce nitrogen monoxide gas

4NH3 + 5O2 4NO + 6H2O

Hafiz Akmal 24

ALLOY

Meaning and purpose of making alloy:-
Alloying is a process of mixing two or more metals (or mixing
metals with element such carbon) which cannot be separated
using physical way

Arrangement of atoms in alloys:-

Pure metal A Pure metal B

Alloys

Hafiz Akmal 25

COMPARE THE HARDNESS OF A PURE
METAL AND ITS ALLOYS

Aim:-
To compare the hardness of a pure metal and its alloy.

Problem Statement:-
Are alloys harder than pure metal ?

Hypothesis:-
Bronze is harder than cooper.

Variables:-
Manipulated: Different types of materials (cooper & bronze)
Responding: diameter of the dent
Controlled: diameter of steel ball bearing, height of the weight,
mass of the weight.

Operational definition:-
1) If the diameter of the dent is smaller, then the material is harder

Materials:-
2) Cooper block, bronze block, cellophane tape

Hafiz Akmal 26

Apparatus:-
3) Retort stand and clamp, 1-kg weight, metre ruler, steel ball
bearing, thread.

Procedure:-
1) A steel ball bearing is taped onto a cooper block using cellophane
tape.
2) A 1-kg weight is hung at a height of 50 cm above the cooper block
as shown in the figure 8.

3) The weight is allowed to drop onto the ball bearing.
4) The diameter of the dent made by the ball bearing on the cooper
block is measured.
5) Steps 1-4 are repeated twice on the other parts of the cooper
block in order to obtain an average value for the diameter of
dents formed.
6) Steps 1-5 are repeated using a bronze block to replace the cooper
block.
7) The reading are recorded in the table.

Hafiz Akmal 27

Results:-

DIAMETER OF THE DENT (mm)
METAL
1 2 3 average
Cooper 2.9 2.8 2.9 2.9
Bronze 2.1 2.2 2.2 2.2

Discussion:-
1) The smaller the diameter of the dent, the harder and stronger is
the material.
2) The average diameter of the dent made on the surface on the
cooper block is bigger than the bronze block.
3) Based on the result, bronze is harder than cooper.

Conclusion:-
The hypothesis is accepted.

Hafiz Akmal 28

EXAMPLE OF ALLOYS

Brass

Stainless
Bronze
Steel

Bronze steel
EXAMPLE
OF ALLOY

Manganese
Steel

Pewter
Stainless steel
Manganese
steel

Hafiz Akmal 29

THE RATE OF RUSTING OF IRON, STEEL,
AND STAINLESS STEEL

Aim:-
To compare the rate of rusting of iron, steel and stainless steel.

Problem statement:-
How does the rate of rusting of iron, steel and stainless steel
differ?

Hypothesis:-
Iron rust faster than steel, and steel rust faster than stainless
steel.

Variables:-
Manipulated variable: Different types of nails
Responding variable: Intensity & amount of blue colour
Controlled variable: Size of nails, concentration of solution used,
durations for rusting.

Operational definition:-
The more intense the blue colour formed, the higher is the rate of
rusting.

Hafiz Akmal 30

Materials:-
Iron nail, steel nail, stainless steel nail, jelly solution, potassium
hexacyanoferrate(lll) solution, water, sandpaper.

Apparatus:-
Test tubes, test tube rack.

Procedure:-
1) The nails are rubbed using sandpaper to remove the rust from the
surface of the nails.
2) The iron nail placed in the test tube A, the steel nail in test tube B
and the stainless steel nail in test tube C.
3) A 5% jelly solution is prepared by adding 5 g of jelly into 100 cm of
boiling water. A few drops of potassium hexacyanoferrate(lll)
solution are then added to the jelly solution.
4) The hot jelly solution is poured into the three test tubes until all
the nails are fully immersed.

5) The test tubes are placed in a test tube rack and left aside for
three days. The intensity of the blue colour is observed.
6) All observation are recorded in the table.

Hafiz Akmal 31

Observation:-

Test tube Intensity of blue colour Inference
A Very High Rusting occurs very fast
B Low Rusting occurs slowly
C Nil No rusting occurs

Discussion:-
1) When iron rust, each iron atom loses two electrons to form an
iron(ll) ion, Fe2+.
Fe (s) = Fe2+ (aq) + 2e- (aq)
2) Potassium hexacyanoferrate(lll) solution is added to the jelly
solution as an indicator to detect iron(ll) ions.
3) When there is iron(ll) ion, potassium hexacyanoferrate(lll)
solution will form dark blue colouration.
4) The higher the intensity of the blue colour, the higher is the rate
of rusting.
5) Solidified jelly solution is used to trap and see the blue
colouration clearly. This is because diffusions occurs the slowest
in solids.
6) Based on the observation, iron rust faster than steel. Stainless
steel does not rust.
7) The nail made from stainless steel does not rust. This is because
this nail is an alloy of iron with carbon, chromium and nickel.

Hafiz Akmal 32

8) The nail made from steel will rust slowly. The presence of carbon
atoms will make the steel stronger than iron but does not prevent
it from rusting.
9) Rusting of iron is an example of corrosion. When corrosion occurs,
the metal loses electrons to form metal iron.

Conclusion:-
Iron rust faster than steel. Stainless steel does not rust.
Hypothesis is accepted.

Hafiz Akmal 33

COMPOSITONS OF ALLOYS & THEIR USES

Alloy Composition Properties Uses
Cu 75% Hard, strong,
Cupronickel Coins
Ni 25% resist corrosion
Al 95%
Aeroplane part, electric cables
Duralumin Cu 4% Light, strong
racing bicycles
Mg 1%
Fe 99% Hard, strong,
Steel Vehicles, bridges, buildings
C 1% cheap
Fe 73%
Kitchen appliance, watches,
Stainless Cr 18% Hard, rust
knifes, fork, spoons, machine
steel Ni 8% resistant
parts
C 1%
Cu 90% Hard, strong, Decorative items, medals,
bronze
Sn 10% shining artwork, pots & pans
Cu 70% Harder and Musical instrument, bell, nails,
Brass
Zn 30% cheaper than Cu screw, and pots
Pb 50% Low melting
Solder Welding, soldering work
Sn 50% point, strong
Sn 91% Malleable,
Pewter Sb 7% ductile, rust Decorative items,souvenirs
Cu 2% resistant
Al 70% Tyre rim of racing car, skeletal
Magnalium Light, strong
Mg 30% body of aeroplane

Hafiz Akmal 34

POLYMER

large molicule
that is in the form
of long chain with
high RMM

POLYMER
made up of many
two types:- monomers which
join together
- natural polymer
through process
- syntetic polymer called
polymerisation

Hafiz Akmal 35

NATURAL POLYMER

Monomer acid Monomer glucose Monomer isoprene
amino Eg: in starch and (2-methylbuta-1,3
Eg: in muscle, skin, cellulose diene)
silk, hairs, wools, and Eg: in latex
furs

Hafiz Akmal 36

SYNTHETIC POLYMER & IT USES
Synthetic polymers are polymers made in industry from chemical
substances.
Many of the raw materials for synthetic polymers are obtained from
petroleum, after refining and cracking process.

Synthetic Synthetic fibres
Thermoplastic
rubber (long chained polymer that withstand
streching)

Nylon (monomers: Polyvinyl chloride(PVC)
Styrene- butadlene
diamine and dicarboxylic (monomers:
rubber (SBR) (monomers:
acid) chloroethene)
styrene & butadlene.
eg:- synthetic eg:- rain clothes, water
eg:- shoe soles & tyres
textile, string pipes

Neoprene (monomers: Terrylene (monomers: Polythene
chloroprene) diol and dicarboxylic (monomers: ethene)
eg:- gloves, electric wire acid) eg:- battery
insulator, water pipes eg:- fishing net cases, pails, plastic bags

Polystytrene
Butyl rubber (monomers:
(monomers:
isobutylene & isoprene)
phenylethene)
eg:- inner tubing of
eg:- toys, disposable cup
tyre, hoses, shoe soles
and plates

Perspex (monomers: Polypropene
methyl metacrylate) (monomers: propene)
eg:- spectacles, car lamps eg:- plastic bottles

Hafiz Akmal 37

WHY USE SYNTETIC POLYMERS IN
DAILY LIFE?

Strong &
light

easily can be made
moulded or to have
shaped & be special
coloured Synthetic properties

polymers

able to resist
cheap
corrosion

Hafiz Akmal 38

ENVIRONMENTAL POLLUTION
RESULTING FROM THE DISPOSAL OF
SYNTHETIC POLYMERS

AIR POLLUTION
- caused by burning of plastic
eg: burning of PVC will
produce dioxin. (dioxin will
destroy human immune
system, reproductive system
& nervous system

Effects of
improper
Disposal of
Synthetic
SOIL POLLUTION Polymer
- plastic thrown on land fill up WATER POLLUTION
our living spaces - plastic will stop the flow of
- destroy the beauty of river water and drains. this
environment will cause flash floods.
-plastic also cause the soil not - plastic also cause the death
suitable for planting because of marine organism if they
plastic inhibit the growth of mistaken the plastic as food.
root

Hafiz Akmal 39

GLASS
Glass:-
The major component of glass is silica or silicon dioxide, SiO2
which found in sand.ri

Impermeable
to liquid

Electrical
Transparent
insulator

Properties
of glass

hard but
Heat insulator
brittle

Chemically
inert

Hafiz Akmal 40

TYPES, COMPOSITION, PROPERTIES, AND
USES OF GLASS

GLASS COMPOSITION PROPERTIES USES
Low melting point Glass container
SiO2 – 70% Mouldable into shapes Glass panes
Na2O – 15% Cheap Mirror
Soda lime glass
CaO – 10% Breakable Lamps and bulbs
Others – 4% Can withstand high Plates and bowls
heat Bottles
High density and Containers for drinks
refractive index and food
SiO2 – 70%
Glittering surface Decorative glass
Lead glass (crystal) Na2O – 20%
Soft Crystal glassware
PbO – 10%
Low melting point Lens for spectacles
(600˚C)
Resistant to high heat Glass apparatus in lab
SiO2 – 80%
&chemical reaction Cooking utensils
Borosilicate glass B2O3 – 13%
Does not break easily
(Pyrex) Na2O – 4%
Allow infra-red rays
Al2O3 – 2%
but no ultra-violet rays
High melting point Scientific apparatus
(1700˚C) like lens on
Expensive spectrometer
SiO2 – 99%
Fused silicate glass Allow ultraviolet to Optical lens
B2O3 – 1%
pass through Lab apparatus
Difficult to melt or
mould into shape

Hafiz Akmal 41

CERAMICS
Ceramics:-
Ceramic is manufactured substances made from clay that is dried,
and heated in a kiln at a very high temperature
The main component of clay is aluminosilicate (aluminum oxide
and silicon dioxide) with small quantities of sand and feldspar.
Unlike glass, ceramic cannot be recycled.
Kaolinite is a high quality white clay that contains hydrated
aluminosilicate, Al2O3•2SiO2•2H2O.

extremely
hard &
strong but
brittle

able to has a very
withstand high
and resist melting
corrosion Properties point
of
ceramics

good
insulator of inert to
electricity chemicals
and heat

Hafiz Akmal 42

THE DIFFERENT CLASES OF CERAMIC

GROUP COMPOSITION
Mineral Quartz – SiO2
Calcite – CaCO3
Cement material Mixture of CaSiO3 and ammonium silicate
Oxide of ceramic Aluminium oxide – Al2O3
Silicon dioxide – SiO2
Magnesium oxide – MgO
Non-oxides of ceramic Silicon nitride – Si3N4
Silicon carbide – SiC
Boron nitride – BN
Boron carbide – B4C3

Hafiz Akmal 43

THE USES OF IMPROVED GLASS AND
CERAMICS FOR SPECIFIC PURPOSES

GLASS OPTICAL FIBRE CONDUCTING GLASS GLASS-CERAMIC CERAMIC PHOTOCHROMIC GLASS
• A pure silica glass thread that • a type of glass that can conduct • Rearrange its atoms into regular SUPERCONUCTOR • sensitive to light intensity
conducts light. electricity. patterns by heating glass to form • superconductor can conduct • the glass darken when exposed
• this fibres can transmit messages • produce by embedding a thin strong material electricity at low temoerature to sunlight but became clear
modulated onto light waves. layer of conducting material in • it can withstand high without resistance, loss of when light intensity decresase.
• used inmedical instrument, LAN glass. temperature, chemical attacks electrical energy as heat • used in windows, sunglasses ad
• adding a layer of indium tin(iv) • used in • used to make light instrument control
oxide (ITO) acts as an electrical tile, cookware, rockets, engine magnet, electric
conductor. blocks motors, electrical generators
• used in the making of LCD

Hafiz Akmal 44

COMPOSITE MATERIALS
A composite material is structural material formed by
combining two or more materials with different physical
properties, producing a complex mixture.
They are used to make various substances in daily life
because of the following reasons:-
a) Metals corrode and are ductile and malleable
b) Glass and ceramic break easily
c) Metal are good conductors but have high resistant,
leading to loss of electrical energy as heat.
d) Plastic and glass can withstand heat to a certain level
only

Hafiz Akmal 45

COMPOSITE PROPERTIES OF PROPERTIES OF
COMPONENT USES
MATERIAL COMPONENT COMPOSITE
concrete hard but brittle stronger construction of road
low tensile strengh higher tensile strength rocket launching pads
does not corrode high-rise buildings
easily
cheaper
Reinforced concrete can be moulded into
shape
steel strong in tensile can withstand very
strength high applied force
expensive can support very
can corrode heavy load

Cooper(ll) oxide Insulator of Conducts electricity Magnetically levitated
Yttrium oxide electricity without resistance train
Superconductor Barium oxide when cooled by liquid Transformer
nitrogen Electric cable
Computer parts
Glass Transparent Reduce refraction of Information display
Not sensitive to light panels
light Control the amount of Light detector device
light passed through it Car windshields
auto. Optical lens
Photochromic glass
Silver chloride Sensitive to light Has the ability to
or silver change colour and
bromide become darker when
exposed to ultraviolet
light
Glass with low Transparent Low material cost Transmit data using
refraction index Does not reflect Reflect light rays and light waves in
light rays allow to travel along telecommunications
the fibre
Fibre optics Can transmit
electronic data or
Glass with
signal, voice and
higher
image
refractive index

glass high density high tensile strength car bodies
strong but brittle moulded and shaped helmets
non-flexible inert to chemicals skies
light, strong, tough rackets
Fibre glass polyester light
non-flammable furniture
plastic flexible
impermeable to water
inflammable
resilient
elastic but weak
flexible

Hafiz Akmal 46

in the medical
field: to replace
organs in the form
of plastic
composite organ

Uses of
composite
material
car part now use
composite material
sronger buildings
instead iron and
are built by using
steel. this increase
reinforce concrete
the speed of the
car and fuel saver

15102759 chemistry-folio-chapter-9-spm

Recomendados

Recomendados

Mais conteúdo relacionado

Mais procurados

Mais procurados (20)

Semelhante a 15102759 chemistry-folio-chapter-9-spm

Semelhante a 15102759 chemistry-folio-chapter-9-spm (20)

Último

Último (20)

15102759 chemistry-folio-chapter-9-spm