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Chemistry in industry Flashcards

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1
Q

What’s a metal ore?

A

Compound with metal found in Earth which is worth extracting

Finite resource

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2
Q

What’s a reduction reaction?

A

A reaction that separates a metal from it’s oxygen

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3
Q

Example of a reduction reaction?

A

Copper oxide + Carbon = Copper + oxygen

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4
Q

Which elements can undergo a reduction reaction with carbon?

A

Anything less reactive than carbon, so the carbon can steal the oxygen

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5
Q

How’s a reduction reaction done?

A

Ore is heated with Carbon monoxide

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6
Q

How are compound ores with more reactive elements than carbon separated?

A

Electrolysis

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7
Q

What’s used to reduce the temperature (and costs), of the electrolysis of aluminium oxide?

A

Cryolite, aluminium oxide has a high boiling point, so instead it’s dissolved in cryolite, making it cheaper and easier

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8
Q

Why does the positive carbon electrode often need replacing?

A

Reacts with oxygen wears it down

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9
Q

What happens at the cathode at the electrolysis of Aluminium oxide?

A

Reduction, the aluminium gains 3 electrons

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10
Q

What happens at the anode at the electrolysis of Aluminium oxide?

A

Oxidation, oxygen loses 4 electrons

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11
Q

What overall reaction is the electrolysis of aluminium oxide?

A

Redox reaction

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12
Q

What’s the complete equation for the decomposition of aluminium oxide?

A

Aluminium Oxide = aluminium + oxygen

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13
Q

Why’s electrolysis expensive?

A

Requires a lot of electricity

Positive electrodes often need replacing

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14
Q

Why’s electrolysis of aluminium good?

A

Now it’s cheap, used to be very rare and hard to extract

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15
Q

How is iron extracted from haematite?

A

Reduction in a blast furnace

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16
Q

What are the raw materials put in the blast furnace?

A

Iron ore, containing the iron
Coke, containing carbon to reduce iron oxide to iron metal
Limestone takes away impurities in the form of slag

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17
Q

How does the iron ore get reduced to iron?

A

Hot air blasted in

Coke burns to produce carbon dioxide

Carbon dioxide reacts with unburnt coke to form carbon monoxide

Carbon monoxide reduces iron ore to iron

iron is molten at this temperature and very dense so it runs down and tapped off at the bottom

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18
Q

How are the impurities removed in a blast furnace?

A

Main impurity is silicon dioxide (sand)

Limestone decomposed by the heat to form calcium oxide and carbon dioxide

Calcium oxide reacts with silicon dioxide to form slag with is molten to tapped off

Slag can be used for road building or fertiliser

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19
Q

What properties do aluminium and iron have in common?

A 
Metals
Dense and shiny
Conduct heat and electricity
Malleable and strong
High boiling points
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20
Q

Use of wrought iron (pure iron)?

A

Malleable so ornamental gates and railings

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21
Q

What’s an alloy?i

A

Irons mixed with another element, giving it different properties

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22
Q

What’s cast iron used for?

A

Hard and brittle, so cooking pans

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23
Q

Steel?

A

Hard, so car bodies

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24
Q

What’s the main problem with iron?

A

It rusts

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25
Q

What’s stainless steel?

A

Alloy of iron and chromium which doesn’t rust

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26
Q

Benefits of aluminium to iron?

A

Doesn’t corrode as layer of aluminium oxide prevents further reactions

Lighter so used in aeroplanes

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27
Q

What’s crude oil?

A

A mixture of Hydro- carbons

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28
Q

How is crude oil separated?

A

Fractional distillation

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29
Q

How does fractional distillation work?

A

Oil is heated up in a fractionating column

Longer Hydrocarbons condense earlier and drain out due to high boiling points

Shorter Hydrocarbons condense later and drain out due to lower boiling points

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30
Q

Features of Refinery gases?

A

Hydrocarbon length: 3

Uses: Bottled gas

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31
Q

Features of gasoline?

A

Hydrocarbon length: 8

Uses: fuel for vehicles

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32
Q

Features of Naphtha?

A

Hydrocarbon length: 10

Uses: Feedstock

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33
Q

Features of Kerosene ( Paraffin)?

A

Hydrocarbon length: 15

Uses: Jet engines

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34
Q

Features of Diesel?

A

Hydrocarbon length: 20

Uses: Fuel for diesel engines

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35
Q

Features of Fuel oil?

A

Hydrocarbon length: 40

Uses: Central heating

36
Q

Features of Bitumen?

A

Hydrocarbon length: 70+

Uses: Road surfaces

37
Q

What happens when fractions from crude oil are burnt as fuels?

A

Pollutants produced

38
Q

Why is carbon monoxide poisonous?

A

Stops red blood cells carrying oxygen, by combining with haemoglobin

39
Q

Why is sulphur dioxide produce from burning fuel?

A

sulphur impurities in the fuel

40
Q

Why are nitrogen oxides produced?

A

Temperature is high enough for Nitrogen and Oxygen to react

41
Q

How does Sulfur dioxide and Nitrogen oxides cause acid rain?

A

Reacts with clouds to form sulphuric acid, or nitric acid

42
Q

Damages of Acid rain?

A

Makes lakes acidic

Damages limestone buildings

43
Q

Features of long Hydrocarbons?

A

High boiling points

44
Q

Features of short Hydrocarbons?

A

Low boiling points

45
Q

What’s cracking?

A

Form of thermal decomposition

46
Q

Why are long Hydrocarbons cracked?

A

The smaller ones are more useful

47
Q

What does cracking also produce?

A

Alkenes used to make polymers

48
Q

How to crack paraffin?

A

Heat the paraffin and make it pass over a heated catalyst in the form of alumina, Paraffin cracks, collect the alkenes

49
Q

Equation for the cracking of a hydrocarbon?

A

Long chain alkane = shorter alkane + alkenes

50
Q

What’s a monomer?

A

The small molecules, with carbon-carbon double bonds (alkenes)

51
Q

How are addition polymers made?

A

When the monomers under go high pressure and a catalyst they join hands (polymerise) to form polymers

52
Q

What’s a polymer?

A

A very long saturated chain

53
Q

What does the N in a polymer equation mean?

A

How many repeat units there are

54
Q

What’s a repeat unit?

A

The part of the polymer which is repeated

55
Q

How do you find the monomer used to form an addition bond?

A

Take the repeat unit and add a double bond

56
Q

What’s a condensation polymer?

A

When 2 monomers react and for each new bond a small molecule (eg water) is lost

57
Q

Example of a condensation polymer?

A

Nylon, Monomer 1 + Monomer 2 = condensation polymer ( nylon) + water

58
Q

Use of poly(ethene)?

A

Stretchable and light so bottles

59
Q

Uses of Poly(propene)?

A

Tough/heat resistant so kettles

60
Q

Uses of Poly(chloroethene)

A

Insulating electrical cables

61
Q

Why are polymers difficult to get rid of?

A

Carbon carbon bonds are tough so they take a long time to bio degrade

62
Q

Why can’t you burn polymers?

A

Release toxic gases

63
Q

Best way to deal with polymers?

A

Reuse them

64
Q

Equation for the harbour process?

A

Nitrogen + Hydrogen = ammonia

65
Q

Use of ammonia?

A

Used as fertiliser

66
Q

Where’s the nitrogen obtained?

A

Air

67
Q

Where’s the hydrogen obtained?

A

Natural gas

68
Q

What’s unique about the harbour process?

A

It’s reversible, so not all ammonia and hydrogen will convert into ammonia, it reaches dynamic equilibrium

69
Q

What are the required conditions for the harbour process?

A

Pressure 200 atmospheres
Temperature 450C
Catalyst Iron

70
Q

Why is the pressure so high in the harbour process?

A

It benefits the forward reaction, so the making of ammonia

71
Q

Why is the temperature 450C

A

Higher temperatures favour the backwards reaction, however increasing the heat makes the reaction faster so it’s a compromise

72
Q

What’s ammonium nitrate a good fertiliser?

A

Provides plants with Nitrogen and ammonia

73
Q

What’s the contact process used for?

A

Making sulphuric acid

74
Q

Describe the contact process?

A

Sulphur is burnt in air to produce sulphur dioxide

Sulphur dioxide is oxidised (with a catalyst) to form sulphur trioxide

Sulfur trioxide is dissolved in concentrated sulphuric acid to form a liquid oleum

Oleum is diluted with water to form concentrated sulphuric acid

75
Q

Why’s a catalyst so important in the contact process?

A

A higher temperature favours the backwards reaction, but a high temperature is needed to increase the speed of the reaction

76
Q

Condition for the contact process?

A

Temperature: 450C
Pressure 2 atmospheres
Catalyst : vanadium oxide

77
Q

Uses of sulphuric acid?

A

Fertilisers
Detergents
Paints

78
Q

What’s produced in the electrolysis of the salt brine ( sodium chloride solution)

A

Hydrogen chlorine and sodium hydroxide

79
Q

Where’s the hydrogen gas given off?

A

Cathode

80
Q

Where’s the chlorine gas given off??

A

Anode

81
Q

Where is the sodium hydroxide produced?

A

Stays in the solution

82
Q

How many electrons are gained or lost by the hydrogen and chlorine?

A

2

83
Q

What’s chlorine used for?

A

Bleach or sterilisation

84
Q

What’s hydrogen used for?

A

Harbour process, or changing oils into fats

85
Q

What’s sodium hydroxide used for?

A

Very strong base, so soap

Chemistry (9 decks)

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