Extraction reactions of metals Flashcards

1
Q

List the methods of extracting a metal from its oxide (3)

A

Displacement reaction with Carbon, Electrolysis, Displacement reaction with another more reactive metal

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2
Q

What will happen in a reaction between Zinc Sulphate + copper

A

No reaction

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3
Q

What will happen in a reaction between Copper Sulfate + Zinc

A

Copper Sulfate + Zinc to Zinc Sulfate + Copper

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4
Q

What is the symbolic equation between Copper Sulfate and Zinc

A

CuSO4+Zn → ZnSO4+ Cu

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5
Q

What is the Termite Reaction+ equation

A

It is displacement, exothermic reaction between Fe2O3+2Al → 2Fe+Al2O3

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6
Q

What is being used to extract iron from its ore?

A

Blast furnace

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7
Q

What chemicals are used for iron extraction?

A

Iron ore is mixed with Coke and Limestone

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8
Q

Why is Limestone being used in the extraction(equation + state symbols)

A

To remove impurities from iron ore. Limestone is decomposed in heat. CaCO3(s) → CaO(s)+CO2(g). Calcium oxide reacts with silicon dioxide which is a main impurity. CaO(s)+SiO2(s) → CaSiO3(l)

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9
Q

What is slag? What happens to it?

A

Calcium silicate (CaSiO3) It float on top of the molten iron and gets removed

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10
Q

Why is Coke burned with oxygen? (equation + state symbols)

A

In order to react with oxygen and form CO2. C(s)+O2(g) → CO2(g)

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11
Q

What happens to carbon dioxide? (Iron extraction stage 2) (equation + state symbols)

A

At high temperatures carbon dioxide is reduced to carbon monoxide CO2(g)+C(s) → 2CO(g)

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12
Q

What happens to carbon monoxide? (Iron extraction part 3) (equation + state symbols)

A

Carbon monoxide reduces the iron in the haematite. Fe2O3(s)+3CO(g) → 2Fe(l) + 3CO2(g)

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13
Q

What is haematite?

A

Iron oxide Fe2O3

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14
Q

What happens to iron as the % of carbon increases? (3)

A

Cost decreases
Becomes more brittle
It becomes softer

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15
Q

When does Iron rust? How can this process be increased?

A

In presence of water and oxygen. Add salt

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16
Q

How to prevent rusting(5)

A
Paint
Coating Oil or grease
Covered with plastic
Alloying
Galvanising
17
Q

What is Alloying of iron

A

Adding Chromium and Nickel to make stainless steel

18
Q

What does alloying do?

A

Provides a strong oxide layer that protects the iron

19
Q

What is Galvanising?

A

Coating with a layer of zinc

20
Q

Why does Galvanising help?

A

Zinc is more reactive than iron, so corrodes instead of iron.

21
Q

What is being used to extract aluminium?

A

Electrolysis

22
Q

What is the overall reaction for extraction of aluminium?

A

2Al2O3 → 4Al+3O2

23
Q

Aluminium oxide has a very high melting point. What is done to it to reduce it?

A

Molten cryolite is added

24
Q

What happens to aluminium ions during electrolysis?(electroe equation)

A

They get attached to cathode and reduced by gaining electrons
AL3+ + 3e- → Al

25
Q

What happens to carbon anodes?

A

They react with oxygen at high temperatures to produce carbon dioxide and have to be replaced every several days

26
Q

Is pure aluminium strong?

A

No

27
Q

What are the advantages of Aluminium (7)

A
Aluminium oxide is strong
It has low density 
Conducts electricity
Resists corrosion 
Has a shiny appearance 
Good strength
Conducts heat
28
Q

What is decomposition?

A

Breaking down of substance into simpler substances