45607824 Folio Chemistry C9 Pt 1

8/8/2019 45607824 Folio Chemistry C9 Pt 1

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ChemistryChapter 9 Folio:Manufactured

Substances InIndustry.

Name : Muhamad Haykal Bin Zol HamidyClass : 4 Ibnu Khaldun

School:MJSC Merbok


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Content Page

1.Introduction

2.Sulphuric Acid

3.Ammonia And Its Salt

4.Alloys

5.Synthetic Polymers

6.Glass And Ceramic

7.Composite Materials


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1.Introduction

In retrospect, the definition of chemistry seems to invariably change per decade, as new

discoveries and theories add to the functionality of the science. Shown below are some of

the standard definitions used by various noted chemists:

Alchemy (330) the study of the composition of waters, movement,

growth, embodying and disembodying, drawing the spirits from bodies and

bonding the spirits within bodies (Zosimos).

Chymistry (1661) the subject of the material principles of mixture bodies

(Boyle).

Chymistry (1663) a scientific art, by which one learns to dissolve bodies, and

draw from them the different substances on their composition, and how to unite

them again, and exalt them to an higher perfection (Glaser).

Chemistry (1730) the art of resolving mixture, compound, or aggregate bodies

into their principles; and of composing such bodies from those principles (Stahl).

Chemistry (1837) the science concerned with the laws and effects of molecular

forces (Dumas).

Chemistry (1947) the science of substances: their structure, their properties, and

the reactions that change them into other substances (Pauling).

Chemistry (1998) the study of matter and the changes it undergoes (Chang).

In the study of matter, chemistry also investigates its interactions with energy anditself.

Because of the diversity of matter, which is mostly composed of different combinations

of atoms, chemists often study how atoms of different chemical elements interact to form

molecules and how molecules interact with each other.


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2.Sulphuric Acid

Properties of sulphuric acid

1.Sulphuric acid is a strong mineral acid

2.Its molecular formula is H2SO4.

3.It is soluble in water.

3.Sulphuric acid is non-volatile diprotic acid.

4.It is a highly corrosive, dense and oily liquid.

5. Concentrated sulphuric acid is a viscous colourless liquid.

A Uses Of Sulphuric Acid.

1) To manufacture fertilizers

a ) Calcium dihydrogen phosphate (superphosphate)

2H 2 SO 4 + Ca 3 (PO 4)2 Ca(H 2 PO 4)2 + 2Ca SO4

Sulphuric acid + tricalcium phosphate calcium dihydrogen phosphate

b) Ammonium sulphate

H2SO4 + 2NH3 (NH4)2 SO4

Sulphuric acid + aqueous ammonia ammonium sulphate

c) Potassium sulphate

K2SO4


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2) To manufacture detergents

Sulphuric acid reacts with hydrocarbon to produce sulphonic acid. Sulphonic acid

is then neutralized with sodium hydroxide to produce detergents.Examples of

hydrocarbon.

3) To manufactured synthetic fibres

Synthetic fibres are polymers (long chain molecules). Rayon is an example of a

synthetic fibre that is produced from the action of sulphuric acid on cellulose.

4) To manufactured paint pigment

The white pigment is paint is usually barium sulphate,BaSO4.The neutralization of

sulphuric acid and barium hydroxide produces barium sulphate.

5) As an electrolyte in lead-acid accumulators.

6) To remove metal oxides from metal surfaces before electroplating.

7) To manufacture pesticides.

8) The uses of sulphuric acid in school laboratories are :

a. As a strong acid.

b. As a drying or dehydrating agent

c. As an oxidizing agent.

d. As a sulphonating agent.

e. As a catalyst.


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The industrial process in manufacture sulphuric acid.

1. Sulphuric acid is manufactured by the Contact process.

2. Sulphuric acid is produced from sulfur, oxygen and water via the contact process.

3. The Contact process involves three stages.

Sulphur Sulphur dioxide Sulphur trioxide Sulphuric acid

I II III

4.Stage I: Production of sulphur dioxide gas, SO2

This can be done by two methods,

a) Burning of sulphur in dry air.

S + O2 SO2

b) Burning of metal sulphide such as zinc sulphide in dry air.

2ZnS + 3O2 2SO2+ 2ZnO

5.Stage II : Conversion of sulphur dioxide to sulphur trioxide SO3.

This is then oxidised to sulfur trioxide under the following conditions:

a ) The presence of a vanadium(V) oxide as a catalyst.

b ) A temperature of between 450C to 550C.c ) A pressure of one atmosphere.

2SO2 + O2 2SO3

6. Stage III : Production of sulphuric acid

a ) Sulphur trioxide is dissolved in concentrated sulphuric acid,H2SO4 to produceoleum, H2S2O7.


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H2SO4 + SO3 H2S2O7

b ) Oleum is reacted with water to form concentrated H2SO4

H2S2O7 + H2O 2H2SO4

7. In stage II, sulphur dioxide is dried first before being added to dry air to

Produce sulphur trioxide. This is :

a ) To remove water vapour

b ) To remove contaminants

8. In stage III, sulphur trioxide is not dissolved directly in water to produce

Sulphuric acid. This is because :

a ) sulphur trioxide has low solubility in water

b ) sulphur trioxide reacts violently and mists are formed instead of a liquid.

The Contact Process


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In The Converter

Sulphur Oxygen

S(s) + O2 (g)SO2(g) 2SO (g) + O2

(g) 2SO3

(g)

Temperature: 450-500C

Pressure: 2-3 atmospheres

Catalyst: Vanadium (V) oxideOxygen

Unreacted2%SO2 is

flowed ba

to converttogether w

SO2

(g) + H2SO

4(aq)H

2S

2O

7

(l)

H2S

2O

7(l) + H

2O (l)2H

2SO

4

(aq)

Outline of Contact process


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SULPHUR DIOXIDE AND ENVIRONMENTAL POLLUTION

1. Sulphur dioxide is one of the by-products of contact process. It is a colourless and

poisonous gas with a very pungent smell.2. Sulphur dioxide which escapes into the air causes air pollution.

3. Sulphur dioxide is an acidic which dissolves in water to form sulphurous acidic,

H2SO3. In the atmosphere, sulphur dioxide dissolve in water droplets to formsulphurous acidic.

SO2 (g) + H2O (l) H2SO3 (aq)

4. Oxidation of sulphur acid by oxygen produces sulphuric acid, H2SO4, which falls to

the earth as acid rain. Sulphur trioxide is also easily oxidised in the air to formsulphur trioxide. Sulphur trioxide dissolve in rainwater to produce sulphuric acid.

SO3 (g) + H2O (l) H2SO4 (aq)

Acid rain and environmental pollution


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3.Ammonia And Its Salts

USES OF AMMONIA

1. Ammonia that is produce commercially has many uses.

2. It uses:

i. In the manufacture of chemical fertilizers such as ammonium sulphate, ammonia

nitric, ammonia phosphate and urea.

ii. To manufacture nitric acid and explosive.

iii. In the making of synthetic fiber and nylon.

iv. As a degreasing agent in aqueous form to remove greasy stains in the kitchen.

Properties Of Ammonia Gas1. The physical properties of ammonia gas include the following:

i. It colourless and has a pungent odour.

ii. It is vary soluble in water and form a weak alkaline solution.

iii. It less dense then water.

iv. It easily liquefied (at about 35.5C) when cool.

2. The chemical properties of ammonia gas:

a) Ammonia gas dissolves in water to form a weak alkali.

NH3 (g) + H2O (l) NH4+ (aq) + OH-(aq)

b) The presence of hydroxide icon causes the aqueous solution to become alkaline.

Thus aqueous ammonia solution:

i. Turns red litmus paper blue.

ii. Reacts with acid to form only salt and waterin neutralization reaction.

NH3(aq) + HCI(aq) NH4CI(aq)

2NH3 + H2SO4(aq) (NH4)2SO4(aq)

iii. Reacts with solution of metallic cations to produce precipitates.

Fe+(aq) + 2OH(aq) Fe (OH)2(s)


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(Form ammonia solution) Dirty green precipitate

MANUFACTURE OF AMMONIA IN INDUSTRY

1. Ammonia is manufacture on a large scale in industry through the Haber process. In

this process, ammonia is formed form direct combination of nitrogen and hydrogen

gas in the volume ratio 1:3.

2. The gas nitrogen obtain form the fractional distillation of liquefied air. The hydrogen

gas is obtained from the cracking of petroleum or from the catalysed reaction of

natural gas, CH4, with steam.

CH4 (g) + H2O (g) CO (g) + 3H2 (g)

3. The mixture of nitrogen and hydrogen gases is passed over an iron catalyst under

controlled optimum condition as below to form ammonia gas.

i. Temperature: 450-500C

ii. Pressure: 200-500 atmospheres

iii. Catalyst used: Iron fillings

N2 (g) + 3H2 (g) 2NH3 (g)

4. Under these control optimum condition, only 15% of the gas mixture turn intoammonia gas. The nitrogen and hydrogen that have not reacted are then flow back over

the catalyst again in the reactor chamber.

5. The ammonia product is then cooled at a low temperature so that it condenses into a

liquid in the cooling chamber.


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The Harber Process

AMMONIUM FERTILIZERS

Nitrogen Hydrogen

N2 and H2 are mixed in the proportion of

1:3In the reactor chamber

N2(g) + 3H

2(g) 2NH

3(g)

Temperature: 450-500C

Pressure: 200-500 atmospheresCatalyst used: Iron fillings

In cooling chamber

Liquid

ammonia

Outline Of Habert process

Unreacted N2 andH2 gases


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1. Nitrogen is required in large amount by plant to make proteins which are necessary

for growth and cell repair.

2. Most plant are not able to get a nitrogen supply directly from the air although it isabundant in the air (78%). Plants can only absorb soluble nitrogen compounds from

soil through their roots.

3. The nitrogen compounds are usually soluble nitric salt, ammonia and ammonia salt

which are manufacture as chemical fertilizer.

4. Reactions of ammonia with acids produce ammonium fertilizers.

NH3(aq) + HNO3(aq) NH4NO3(aq)

Ammonium nitrate

3NH3(aq) + H3PO4(aq) (NH4)3PO4(aq)

Ammonium phosphate

2NH3(aq) +H2SO4(aq) (NH4)2SO4(aq)

4.Alloys.


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ARRANGEMENT OF ATOMS IN METALS

1. The atom of pure metals is packed together closely. This causes the metal to have a

high density

2. The forces of attraction between atoms (metallic bonds) are strong. More heat

energy is needed to overcome the metallic bond so that the atoms are further apart

during the melting. This is why metals usually have high melting point.

3. Heat energy can be transferred easily from one atom to the next by vibration. This

makes metal good conduct of heat.

4. The freely moving outermost electrons within the metals structure are able toconduct electricity. Metal are, therefore, good electrical conductors.

5. Since atoms of pure metal are of the same size, they are arranged orderly in a regular

layered pattern. When a force is applied to metal, layer of atom slide easily over one

another. This makes pure metals soft, malleable and ductile.


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Matel are malleable

ce

Metals are ductile

ceThe shape of the

metal change

45607824 Folio Chemistry C9 Pt 1

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