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Chemistry > Chapter 4 - Extracting Metals and Equilibria > Flashcards

Chapter 4 - Extracting Metals and Equilibria Flashcards

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1
Q

Reactivity series.

A

Potassium, Sodium, Calcium, Magnesium, Aluminum, CARBON, Zinc, Iron, HYDROGEN, Copper, Silver, Gold

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2
Q

Below hydrogen on series

A

Doesn’t react with dilute acids

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3
Q

Metals at the top

A

More easily oxidise to form cations.

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4
Q

Testing reactivity

A

Add metals to acid, perform squeaky pop test. The louder the more reactive as reaction rate is higher meaning more H2 per second.

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5
Q

Metal + water
(Reactive metals)
Metal + steam
(Less reactive)

A

Metal Hydroxide + Hydrogen

Metal Oxide + Hydrogen

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6
Q

Displacement reactions are examples of..

A

REDOX reactions.
More reactive - oxidation
Less reactive - reduced

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7
Q

Displacement reactions define

A

More reactive metals take the place of less reactive metals

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8
Q

Metals are found in

A

Ores

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9
Q

Aluminium ore

A

Bauxite Al2O3

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10
Q

What can be extracted using carbon?

A

Metals less reactive than iron can be reduced in a blast furnace.

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11
Q

Metals more reactive carbon must be extracted using

A

Electrolysis

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12
Q

Why electrolysis is expensive

A

Large amounts of electricity is expensive.
If the ore must be melted

Reduction with carbon is cheaper as carbon is cheap and fuels the heat in an exothermic reaction

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13
Q

Bioleaching

A

Uses bacteria to separate metals from ores. Bacteria carry out chemical reactions and form a leachate, contains high concentration of metals. This can be extracted using electrolysis or displacement.

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14
Q

Phytoextraction

A

Plants grown on soil with metal compounds. They are taken up and build up in tissue. They are burned forming ash with metals, extracted using electrolysis or displacement

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15
Q

Recycling positives

A

Prevents finite resources running out
Saves more energy than original extraction
Mines are damaging to environment and destroy habitat.
Reduces landfill.

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16
Q

Economic benefits of extraction

A

Extracting costs more than recycling.

Creates jobs

17
Q

Life Cycle Assesment

A

LCA , looks at every stage of the lifetime of a product

18
Q

LCA: Choice of material

A

Metals must be mined and extracted requiring energy, releasing pollution .
Crude oil is non-renewable and requires lots of energy in extraction

19
Q

LCA: Manufacturing

A

Uses lots of energy
Causes pollution
Waste may be poorly disposed
Often require water, contaminated water may be let out.

20
Q

LCA: Product Use

A

Burning fuels releases

Fertilisers can leach into water causing damage to ecosystem.

21
Q

LCA: Disposal

A

May be disposed in Landfill, polluting land and water.

Products may be incinerated causes air pollution.

22
Q

Haber process equation

A

N2 + 3H2 2NH3

23
Q

Haber process temperature, pressure and catalyst

A

450C,
200 atmospheres
Iron catalyst

24
Q

Dynamic equilibrium

A

The forward and backward reactions are happening at the same rate and time. Concentrations have reached a balance so won’t change.

25
Q

Equilibrium can only be reached in a

A

Closed System

26
Q

Equilibrium shifts right

A

More products (concentration) less reactant (concentration)

27
Q

Equilibrium shifts left

A

More reactant (concentration) Less products (concentration)

28
Q

What 3 things can change the position of equilibria.

A

Temperature,
Pressure (involving gases)
Concentrations (reactants or products)

29
Q

Effect of temperature on equilibria.

A

Increase : Moves ENDOthermic direction.

Decrease: Moves EXOthermic direction

30
Q

Le Chatelier principle

A

If the concentration, temperature or pressure change, the reaction will shift to COUNTERACT this.

31
Q

Changing pressure on equilibria

A

Increasing: Moves side with few moles of GAS
Decreasing: Moves to side with more moles of GAS

32
Q

Changing concentration on equilibria

A

Increase REACTANTS: Shifts right, to use up the added reactants.

Increase PRODUCTS: Shifts Left to use up the added products.

Decreasing has the OPPOSITE effect.

Chemistry (7 decks)

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