Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry > Chapter 4 - Extracting Metals and Equilibria > Flashcards

Chapter 4 - Extracting Metals and Equilibria Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

Reactivity series.

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Below hydrogen on series

A

Doesn’t react with dilute acids

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Metals at the top

A

More easily oxidise to form cations.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

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

A

Metal Hydroxide + Hydrogen

Metal Oxide + Hydrogen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Displacement reactions are examples of..

A

REDOX reactions.
More reactive - oxidation
Less reactive - reduced

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Displacement reactions define

A

More reactive metals take the place of less reactive metals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Metals are found in

A

Ores

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Aluminium ore

A

Bauxite Al2O3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What can be extracted using carbon?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Metals more reactive carbon must be extracted using

A

Electrolysis

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions