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Chemistry Revision > Chemistry In Industry (Metals, Iron, Aluminium) > Flashcards

Chemistry In Industry (Metals, Iron, Aluminium) Flashcards

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1
Q

Most metals are found in _______

A

Ores

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2
Q

Metals often have to be separated from their ________

A

Oxides

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3
Q

Metals above carbon in the reactivity series are extracted by what method

A

Electrolysis

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4
Q

Metals below carbon in the reactivity series are extracted by what method

A

Heating with carbon monoxide

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5
Q

What is used in the electrolysis of aluminium

A

Molten cryolite

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6
Q

Why is molten cryolite used in the electrolysis of aluminium

A

The aluminium oxide dissolves in it and brings the temperature down to about 900C

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7
Q

Aluminium is extracted from aluminium oxide. Why does molten aluminium oxide conduct electricity

A

Because it has free ions

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8
Q

Electrolysis of aluminium oxide:
Positive Al3+ ions are attracted to the negative electrode (________)
The negative O2- ions are attracted to the positive electrode (________)

A

Cathode

Anode

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9
Q

Why does the positive anode often need repacing

A

By getting worn down by the oxygen

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10
Q

Half equation of aluminium oxide a the cathode:

A

Al3+ + 3e- –> Al

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11
Q

Half equation of aluminium oxide at the anode:

A

2O2- –> O2 + 4e-

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12
Q

Complete equation for the decomposition of aluminium oxide

A

Aluminium oxide –> Aluminium + Oxygen

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13
Q

Why is electrolysis expensive

A

Lots of electricity used

Replacement of positive electrodes (anode) needed

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14
Q

What are the raw materials in the extraction of iron

A

Iron ore
Coke
Limestone

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15
Q

What is coke and what does it do

A

Almost pure carbon (reduces the iron oxide to iron metal)

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16
Q

What does limestone do

A

Limestone takes away impurities in the form of slag

17
Q

What is the first step in the reduction of iron ore to iron

A

Hot air is blasted in, making the coke burn faster than usual. This raises the temperature to about 1500C

18
Q

The coke burns and produces Carbon dioxide.

What is the equation for this

A

C + O2 –> CO2

Carbon + Oxygen –> Carbon dioxide

19
Q

The Co2 then reacts with the unburnt coke form CO.

What is the equation for this

A

CO2 + C –> 2CO

Carbon dioxide + Carbon –> Carbon monoxide

20
Q

The carbon monoxide then reduces the iron ore to iron.

What is the equation for this

A

3CO + Fe2O3 –> 3CO2 + 2Fe

Carbon monoxide + Iron (|||) oxide –> Carbon dioxide + Iron

21
Q

What is the main impurity in the blast furnace

A

Sand (Silicon dioxide)

22
Q

What removes the silicon dioxide

A

Limestone

23
Q

The limestone is decomposed by the heat into calcium oxide and CO2.
What is the equation for this

A

CaCO3 –> CaO + CO2

24
Q

The calcium oxide then reacts with the sand to form calcium silicate (slag), which is molten and can be tapped off.
What is the equation for this

A

CaO + SiO2 —> CaSio3 (molten slag)

25
Q

What can cooled slag be used for?

A

Road building

Fertiliser

26
Q

Describe how iron is produced from iron ore coke in the blast furnace

A

The coke burns (with oxygen) to produces CO2
The Co2 reacts with the unburnt coke to form CO
The CO reduces the iron ore to iron (+ CO2)

27
Q

Properties of both iron and aluminium:

A 
They both:
Are dense
Are good conductors of heat and electricity
Are malleable
Are strong
Have high melting points
28
Q

What is wrought iron and what are its uses

A

Pure iron

Gates, railing

29
Q

You can mix iron with other elements to make _______

A

Alloys

30
Q

Stainless steel is an alloy of iron. What can it be used for

A

Cutlery, cooking pans

31
Q

What is the main problem with iron

A

It rusts

32
Q

What is aluminium used for

A

Aeroplanes

Drink Cans

33
Q

What makes aluminium more suited for aeroplanes than iron

A

It doesn’t corrode

It is lighter (less dense)

Chemistry Revision (9 decks)

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