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sulphuric acid is a diprotic (dibasic) mineral acid which does not volatise. In the pure, concentrated form, sulphuric acid is an oily, colourless liquid which is dense and viscous. It has high boiling point, that is 270 ˚C Hafiz Akmal CHEMISTRY FOLIO chapter 9: Manufacture Substances in industry 1 SULPHURIC ACID
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Page 1: Chemistry

sulphuric acid is a diprotic (dibasic)

mineral acid which does not volatise.

In the pure, concentrated form,

sulphuric acid is an oily, colourless liquid which is dense and viscous.

It has high boiling point, that is 270 ˚C

Hafiz AkmalCHEMISTRY FOLIO chapter 9: Manufacture Substances in industry

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SULPHURIC ACID

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USES OF SULPHURIC ACID

Figure 1:- Uses of Sulphuric Acid, H2SO4

sulphuric acid: making fertiliser

superphosphate fertilisers :- - it is

manufactured from the reaction between sulphuric

acid and calcium phosphate.

Ammonia Sulphate fertiliser:- - It is manufactured by the

neutralisation of sulphuric acid and ammonia

Potassium Sulphate:- - It is manufactured by the

neutralisation of sulphuric acid potassium hydoxide

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

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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:-

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

Stage 1: The production of sulphur dioxide

Stage 2: Formation of sulphur trioxide

Stage 3: Formation of sulphuric acid

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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)

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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)

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)

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b) The reaction takes place in a heat converter.c) Excess air is used to ensure higher percentage of SO3 produced.

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)

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Sulphur

Sulphur dioxide SO2

Sulphur trioxide SO3

Oleum H2S2O7

concentated sulphuric acid, H2SO4

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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.

CONTACT PROCESS:

Burnt in air

O2 , V2O5, 450˚C, 1 atm

Concentrated H2SO4

Water

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Figure 2:- Flow chart of Contact Process

The

indu

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l pro

cess

in th

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of S

ulph

uric

Aci

d

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To manufacture nitrogenous

fertilisers

As a cooling agent

To prevent the coagulation of latex in the rubber industry

To manufacture nitric acid in industry

To manufacture explosive

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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 reaction involved are as the following: a) 2NH3 (g) + H2SO4 (aq) (NH4)2SO4 (s) ammonium sulphate 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 cooling agent in refrigerators and air conditioners.

It neutralizes the organic acids formed by microorganisms in latex, thereby preventing coagulation and preserving the latex in liquid form.

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.4NH3 (g) + 5O2 (g) Pt/900˚C 4NO (aq) + 6H2O (l)

2) nitrogen monoxide is further oxidised to nitrogen

The

indu

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l pro

cess

in th

e M

anuf

actu

red

of S

ulph

uric

Aci

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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:-

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.4NH3 (g) + 5O2 (g) Pt/900˚C 4NO (aq) + 6H2O (l)

2) nitrogen monoxide is further oxidised to nitrogen

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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

3. The mixture is heated4. 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:

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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.

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.

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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.

Observation :-

Section Observation Inference

b)

pH of ammonia solution is 10

pH of sodium hydroxide solution is 14

ammonia is weak alkali

sodium hydroxide is a strong alkali

c)

colourless gas pungent smell water rushed up

and fills up the whole test tube

ammonia is a colourless gas with a pungent smell

ammonia is very soluble in water

d) moist red litmus paper on top of the upright test tube does not change colour.

Ammonia gas has escaped from the upright test tube and thus is slightly less dense than air

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Moist red litmus paper under the inverted test tube turns blue

e) Dense white fumes are formed

Ammonia react with hydrogen chloride gas to form ammonium chloride

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 hydroxideNH3 (g) + H2O (l) = NH4

+ (aq) + OH- (aq) Ammonia is slightly less dense than air Ammonia react with hydrogen chloride gas to form ammonium

chlorideNH3 (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

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hydrogen chloride gas to form dense white fumes of ammonium chloride

HABER PROCESS

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The

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ufac

ture

of a

mm

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thro

ugh

the

Hab

er P

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ss

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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:-

The

man

ufac

ture

of a

mm

onia

thro

ugh

the

Hab

er P

roce

ss

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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.

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.

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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.

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.

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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

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.

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Conclusion:-

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

THE PHYSICAL PROPERTIES OF PURE METAL

THE PHYSICAL PROPERTIES OF

PURE METAL

Ductile

Malleable

High DensityGood Conductor

High Melting & Boiling point

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PROPERTIES OF AMMONIA

alkaline gas, colurless and pungent gas

Ammonia turns the damp red litmus paper blue.

The gas is less dense than air

NH3 + H2O NH4+ OH-

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.

2NH3 + H2SO4 (NH4)2SO4 Ammonia gas burns in oxygen to produce nitrogen monoxide gas

4NH3 + 5O2 4NO + 6H2O

An inverted filter funnel is used to prevent sucking back of water

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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

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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:-

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2) Cooper block, bronze block, cellophane tape

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.

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6) Steps 1-5 are repeated using a bronze block to replace the cooper block.

7) The reading are recorded in the table.

Results:-

METALDIAMETER OF THE DENT (mm)

1 2 3 averageCooper 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.

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EXAMPLE OF ALLOYS

EXAMPLE OF ALLOY

Brass

Stainless Steel

Manganese steel

Manganese Steel

Bronze

Stainless steel

steel

Pewter

Bronze

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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:-

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The more intense the blue colour formed, the higher is the rate of rusting.

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.

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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.

Observation:-

Test tube Intensity of blue colour InferenceA Very High Rusting occurs very fastB Low Rusting occurs slowlyC 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) Based on the observation, iron rust faster than steel. Stainless steel does not rust.

6) The nail made from stainless steel does not rust. This is because this nail is an alloy of iron with carbon, chromium and nickel.

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7) 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.

8) 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.

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COMPOSITONS OF ALLOYS & THEIR USES

Alloy Composition Properties UsesCupronickel

Cu 75%Ni 25%

Hard, strong, resist corrosion

Coins

DuraluminAl 95%Cu 4%Mg 1%

Light, strongAeroplane part, electric cables racing bicycles

SteelFe 99%

C 1%Hard, strong, cheap

Vehicles, bridges, buildings

Stainless steel

Fe 73%Cr 18%Ni 8%C 1%

Hard, rust resistant

Kitchen appliance, watches, knifes, fork, spoons, machine parts

bronzeCu 90%Sn 10%

Hard, strong, shining

Decorative items, medals, artwork, pots & pans

BrassCu 70%Zn 30%

Harder and cheaper than Cu

Musical instrument, bell, nails, screw, and pots

SolderPb 50%Sn 50%

Low melting point, strong

Welding, soldering work

PewterSn 91%Sb 7%Cu 2%

Malleable, ductile, rust resistant

Decorative items,souvenirs

MagnaliumAl 70%

Mg 30%Light, strong

Tyre rim of racing car, skeletal body of aeroplane

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POLYMER

POLYMER

large molicule that is in the form of long chain

with high RMM

made up of many monomers which join

together through process called polymerisation

two types:-- natural polymer- syntetic polymer

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NATURAL POLYMER

Natural polymer

Protein Carbohydrates Natural Rubber

Monomer acid amino

Eg: in muscle, skin, silk, hairs, wools, and furs

Monomer glucose Eg: in starch and

cellulose

Monomer isoprene(2-methylbuta-1,3 diene)

Eg: in latex

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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 rubber

Styrene- butadlene rubber (SBR) (monomers:

styrene & butadlene.eg:- shoe soles & tyres

Neoprene (monomers: chloroprene)

eg:- gloves, electric wire insulator, water pipes

Butyl rubber (monomers: isobutylene & isoprene)eg:- inner tubing of tyre,

hoses, shoe soles

Perspex (monomers: methyl metacrylate)

eg:- spectacles, car lamps

Synthetic fibres(long chained polymer that withstand

streching)

Nylon (monomers: diamine and dicarboxylic

acid)eg:- synthetic textile,

string

Terrylene (monomers: diol and dicarboxylic acid)

eg:- fishing net

Thermoplastic

Polyvinyl chloride(PVC) (monomers:

chloroethene)eg:- rain clothes, water

pipes

Polythene (monomers: ethene)

eg:- battery cases, pails, plastic bags

Polystytrene (monomers: phenylethene)

eg:- toys, disposable cup and plates

Polypropene (monomers: propene)

eg:- plastic bottles

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WHY USE SYNTETIC POLYMERS IN DAILY LIFE?

Synthetic polymers

Strong & light

can be made to have special properties

cheapable to resist corrosion

easily moulded or shaped & be

coloured

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ENVIRONMENTAL POLLUTION RESULTING FROM THE DISPOSAL OF

SYNTHETIC POLYMERS

Effects of improper Disposal of

Synthetic Polymer

AIR POLLUTION- caused by burning of plastic

eg: burning of PVC will produce dioxin. (dioxin will destroy human immune

system, reproductive system & nervous system

WATER POLLUTION- plastic will stop the flow of river water

and drains. this will cause flash floods. - plastic also cause the death of marine organism if they mistaken the

plastic as food.

SOIL POLLUTION- plastic thrown on land fill up our living

spaces - destroy the beauty of environment -plastic also

cause the soil not suitable for planting because plastic inhibit the growth of root

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GLASSGlass:-

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

Properties of glass

Impermeable to liquid

Electrical insulator

Heat insulator

Chemically inert

hard but brittle

Transparent

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TYPES, COMPOSITION, PROPERTIES, AND USES OF GLASS

GLASS COMPOSITION PROPERTIES USES

Soda lime glass

SiO2 – 70%Na2O – 15%CaO – 10%

Others – 4%

Low melting point Mouldable into shapes Cheap Breakable Can withstand high

heat

Glass container Glass panes Mirror Lamps and bulbs Plates and bowls Bottles

Lead glass (crystal)SiO2 – 70%Na2O – 20%PbO – 10%

High density and refractive index

Glittering surface Soft Low melting point

(600˚C)

Containers for drinks and food

Decorative glass Crystal glassware Lens for spectacles

Borosilicate glass (Pyrex)

SiO2 – 80%B2O3 – 13%Na2O – 4%Al2O3 – 2%

Resistant to high heat &chemical reaction

Does not break easily Allow infra-red rays

but no ultra-violet rays

Glass apparatus in lab Cooking utensils

Fused silicate glassSiO2 – 99%B2O3 – 1%

High melting point (1700˚C)

Expensive Allow ultraviolet to

pass through Difficult to melt or

mould into shape

Scientific apparatus like lens on spectrometer

Optical lens Lab apparatus

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CERAMICSCeramics:-

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.

Properties of ceramics

extremely hard & strong but

brittle

has a very high melting point

inert to chemicals

good insulator of electricity and

heat

able to withstand and

resist corrosion

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THE DIFFERENT CLASES OF CERAMIC

GROUP COMPOSITIONMineral Quartz – SiO2

Calcite – CaCO3

Cement material Mixture of CaSiO3 and ammonium silicateOxide of ceramic Aluminium oxide – Al2O3

Silicon dioxide – SiO2

Magnesium oxide – MgO Non-oxides of ceramic Silicon nitride – Si3N4

Silicon carbide – SiC Boron nitride – BNBoron carbide – B4C3

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THE USES OF IMPROVED GLASS AND CERAMICS FOR SPECIFIC PURPOSES

GLASS OPTICAL FIBREA pure silica glass thread that conducts light.this fibres can transmit messages modulated onto light waves.used inmedical instrument, LAN

CONDUCTING GLASSa type of glass that can conduct electricity.produce by embedding a thin layer of conducting material in glass.adding a layer of indium tin(iv) oxide (ITO) acts as an electrical conductor.used in the making of LCD

GLASS-CERAMICRearrange its atoms into regular patterns by heating glass to form strong materialit can withstand high temperature, chemical attacksused in tile, cookware, rockets, engine blocks

CERAMIC SUPERCONUCTORsuperconductor can conduct electricity at low temoerature without resistance, loss of electrical energy as heatused to make light magnet, electric motors, electrical generators

PHOTOCHROMIC GLASSsensitive to light intensitythe glass darken when exposed to sunlight but became clear when light intensity decresase.used in windows, sunglasses ad instrument control

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Hafiz AkmalCHEMISTRY FOLIO chapter 9: Manufacture Substances in industry

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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 malleableb) Glass and ceramic break easilyc) 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

Page 44: Chemistry

Hafiz AkmalCHEMISTRY FOLIO chapter 9: Manufacture Substances in industry

44

COMPOSITE MATERIAL

COMPONENT PROPERTIES OF COMPONENT

PROPERTIES OF COMPOSITE

USES

Reinforced concrete

concrete hard but brittle low tensile strengh

stronger higher tensile strength does not corrode

easily cheaper can be moulded into

shape can withstand very

high applied force can support very

heavy load

construction of road rocket launching pads high-rise buildings

steel strong in tensile strength

expensive can corrode

Superconductor

Cooper(ll) oxide Yttrium oxide Barium oxide

Insulator of electricity

Conducts electricity without resistance when cooled by liquid nitrogen

Magnetically levitated train

Transformer Electric cable Computer parts

Photochromic glass

Glass Transparent Not sensitive to

light

Reduce refraction of light

Control the amount of light passed through it auto.

Has the ability to change colour and become darker when exposed to ultraviolet light

Information display panels

Light detector device Car windshields Optical lens

Silver chloride or silver bromide

Sensitive to light

Fibre optics

Glass with low refraction index

Transparent Does not reflect

light rays

Low material cost Reflect light rays and

allow to travel along the fibre

Can transmit electronic data or signal, voice and image

Transmit data using light waves in telecommunications

Glass with higher refractive index

Fibre glass

glass high density strong but brittle non-flexible

high tensile strength moulded and shaped inert to chemicals light, strong, tough non-flammable impermeable to water resilient flexible

car bodies helmets skies rackets furniture polyester plastic light

flexible inflammable elastic but weak