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Chemistry > C6.1 > Flashcards

C6.1 Flashcards

1
Q

What is a fertiliser?

A
  • chemical or natural substance added to soil or land to improve growth of plants
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2
Q

How must nitrogen be for plants to absorb it?

A
  • as a soluble nitrate not in the air
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3
Q

Formula for Ammonium Sulfate?

A
  • 2NH3 + H2SO4 -> (NH4)2SO4
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4
Q

How can you make ammoinium sulfate in the lab?

A
  • using titration
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5
Q

What are the 3 important elements for plants and what are they called?

A
  • Nitrogen
  • Potassium
  • Phosphorus
  • called NPK and macronutrients
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6
Q

What is phosphorus needed for in a plant?

A
  • to promote strong roots and fruit development
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7
Q

What is potassium needed for in a plant?

A
  • to promote healthy growing in general
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8
Q

Why is nitrogen needed in a plant?

A
  • used to make chlorophyll
  • used to make amino acids
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9
Q

Are Potassium salts all soluble?

A

YES

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10
Q

How to make ammonium phosphate

A
  • Phosphate Rock + Nitric Acid -> Phosphoric Acid + Calcium Nitrate
  • Phosphoric Acid + Ammonia -> Ammonium Phosphate (NH4)3PO4
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11
Q

Differences between lab and industrial prep?

A
  • small scale in lab, large scale industrial
  • safe using dilute concentrations of acids and alkali, danger of explosion as high temp and pressure
  • glass equipment, stainless steel to withstand harsh conditions
  • done at room temp, done at high temp and pressure
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12
Q

Reaction of phosphate rock and sulphuric acid?

A
  • mix of calcium phosphate and calcium Sulfate (called single superphosphate)
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13
Q

Reaction of phosphate rock and phosphoric acid?

A
  • called triple superphosphate and is calcium phosphate
  • fertiliser
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14
Q

What is the industry method for producing ammonia?

A
  • the Haber Process
  • Nitrogen + Hydrogen <-> Ammonia
  • N2 + 3H2 -> 2NH3
  • reversible
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15
Q

Where does the nitrogen for the Haber process come from?

A

From the air, as the air is 79% Nitrogen

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16
Q

How does the Haber Process work?

A
  • the pure reactants are fed into a compressor (200 A and 450oc)
  • then fed into reaction vessel with an iron vessel where the reaction takes place
  • sent to a cooling chamber and liquid ammonia is taken away while any unreacted reactants and heat are recycled
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17
Q

In the Haber Process is the forwards reaction endo or exo?

A
  • in the Haber process the forwards reaction is exo
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18
Q

Why do we use a high pressure for the Haber Process?

A
  • since there is less moles/molecules on the product side so increasing the pressure will mean increased forwards reaction
  • as the system will try and counteract the change
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19
Q

Why do we use 450oc for the Haber Process

A
  • we need to balance the need for a high rate of reaction and the fact that higher temperatures will favour the backwards reaction, decreasing yield
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20
Q

Why is the ammonia formed from the Haber Process removed as the reaction continues?

A
  • to decrease concentration of the product which means equilibrium position will sift to the right and produce more ammonia
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21
Q

What is the contact process?

A
  • the industrial process of making sulphuric acid
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22
Q

What are the raw materials of the Contact Process?

A
  • sulfur
  • air (provides oxygen)
  • water
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23
Q

What is Stage 1 of the Contact Process?

A
  • Sulfur + Oxygen (from air) -> Sulfur Dioxide
  • S + O2 -> SO2
  • exothermic
  • not reversible
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24
Q

What is Stage 2 of the Contact Process?

A
  • Sulfur Dioxide (from Stage 1) + Oxygen <-> Sulfur Trioxide
  • 2SO2 + O2 <-> 2SO3
  • exothermic for the forward reaction
  • uses Vanadium Oxide catalyst
  • 200,00 Pa pressure
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25
Q

What is Stage 3 of the Contact Process?

A
  • Sulfur Trioxide + Water -> Sulphuric Acid
  • SO3 + H2O -> H2SO4
  • very exothermic
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26
Q

What are the 2 substages of Stage 3 of the Contact process?

A
  • there are 2 substages as the onestep reaction is extremely exothermic and very dangerous
    1. H2SO4 + SO3 -> H2S2O7
  • first dissolved in pre-made sulphuric acid
    2. H2S2O7 + H20 -> 2H2SO4
  • The Oleum is mixed with water to give Sulphuric Acid
27
Q

Uses of Sulphuric Acid?

A
  • Fertilisers
  • Extracting Metals
  • Paints
  • Plastics
  • Cleaning Products
  • Car Batteries
28
Q

What is the minimum temp for catalyst in the Contact Process

A
  • Vanadium Oxide
  • 380Oc
29
Q

What are the uses of ethanol?

A
  • fuels
  • alcohol
  • solvent
  • handwash
  • perfume
30
Q

Fermentation to produce ethanol?

A
  • Glucose -> Ethanol + Carbon Dioxide (also uses Yeast)
  • C6H12O6 -> 2C2H5OH + 2CO2
  • glucose come from plant sugars
31
Q

Optimum Temperature for Fermentation?

A

35oC

32
Q

Ethene way to make ethanol?

A
  • Ethene + Steam <-> Ethanol
  • C2H4 + H2O <-> C2H5OH
  • 100% Atom Economy
  • exothermic
33
Q

Best Conditions for producing Ethanol using Ethene

A
  • High Pressure (60 At)
  • Medium Temperature (300oC) (balances RoR and Yield
34
Q

What is the catalyst for producing ethanol from steam?

A

Phosphoric Acid

35
Q

Comparing Fermentation and Ethene Methods

A

Ethene:
- Non-Renewable Raw Materials
- High Temperature
- High Pressure
- Large Amounts of energy needed
- Fast Rate of Reaction
- High Yield (95%)
- High Purity

Fermentation:
- renewable raw materials
- low temperature
- normal pressure
- not much energy required
- slow RoR
- low yield (15%)
- low purity

36
Q

How do we get low reactivity metals?

A
  • they are found naturally pure so we can just dig them up
  • e.g Gold, Platinum and Silver
37
Q

What are Ores?

A

Metal Compounds found in Rock

38
Q

How do we extract metals less reactive than carbon?

A
  • We use displacement and since carbon is more reactive it will displace these metals from their compounds
  • e.g zinc, iron, copper, silver etc.
  • reduction with carbon
39
Q

What are the raw materials for extracting iron?

A
  • Limestone (calcium carbonate, CaCO3)
  • Iron Ore (Haematite)
  • Coke (form of carbon)
  • Hot Air
40
Q

What is the first reaction in Extracting Iron

A
  • Carbon + Oxygen -> Carbon Dioxide
  • C + O2 -> CO2
  • Combustion reaction, helps keep high temp of furnace
41
Q

What is the second reaction in Extracting Iron

A
  • Carbon + Carbon Dioxide -> Carbon Monoxide
  • C + CO2 -> 2CO
  • Carbon Monoxide produced as the reducing agent to displace iron
42
Q

What is the third reaction in Extracting Iron

A
  • Carbon Monoxide + Iron Oxide -> Carbon Dioxide + Iron
  • CO + Fe2O3 -> CO2 + 2Fe
  • redox reaction
43
Q

What is the limestone used for in extracting iron?

A

To react with impurities in the ore to make the iron more pure
- Calcium Carbonate (limestone) -> Calcium Oxide + Carbon Dioxide
- thermal decomposition
- Calcium Oxide + Silica(sand)-> Calcium Silicate (slag)
- neutralisation

44
Q

How pure is the iron from the extraction of iron

A
  • about 95-97% pure
45
Q

What is the ore of aluminium

A

BAUXITE

46
Q

What is the ore of aluminium purifed into

A
  • aluminium oxide
47
Q

For the electrolysis of Aluminium Oxide (AL2O3) what are the cathodes made of?

A
  • GRAPHITE (CARBON), conducts electricity and is unreactive
48
Q

What is cryolite and why is it used in the electrolysis of Aluminium Oxide?

A
  • the aluminium oxide dissolves into cryolite
  • this means the molten electrolysis can take place at a lower temp as cryolite’s melting point is lower than aluminiums
  • this means it is more efficient
49
Q

What happens to the oxygen bubbles at the anode in extracting aluminium?

A
  • They react with the carbon anode and from carbon dioxide
50
Q

What is Phytoextraction?

A
  • this is where plants are grown on the low grade ore
  • the plant’s take up the copper ions
  • the plants are harvested and burnt
    -The ash can be made into metal/copper sulfate solution
51
Q

What is Bioleaching?

A
  • Bacteria is used to break down the metal compounds in the soil
  • this produces a solution of metal salt which can be purified into metal
52
Q

Advantages of Biological Methods of Extraction?

A
  • Removes toxic compounds from the soil
  • mining not required
  • less waste rock
  • less energy needed
53
Q

Disadvantages of Biological Methods of Extraction?

A
  • slow
  • copper is still not pure, needs further purification
54
Q

Advantages and disadvantages of extracting high grade ores with reduction with carbon

A

+ Higher percentage of copper produced
- Finite/running out of ore
- Expensive/ Energy consuming
- Damaging to the environment

55
Q

What is corrosion?

A
  • The destruction of materials by chemical reactions with substances in the environment
  • generally refers to metals
56
Q

What happens with corrosion in iron?

A
  • Rust forms which is iron oxide which flakes off the metal leaving more and more metal exposed
  • until the metal breaks
57
Q

Conditions for Rust?

A
  • Water / H20
  • Air / O2
58
Q

How can you prevent rust (barrier):

A
  • Use the barrier method
  • coat the metal in something else to protect it
  • e.g Paint
  • Oil/Grease
  • Plastic
  • Less Reactive Metal
59
Q

What is the second method of protecting against rust? (Sacrificial)

A
  • more reactive metal protects the iron more effectively
  • with zinc it is called galvanising
  • the more reactive metal will react with the water/oxygen instead of the iron
  • If rust does form it is displaced away by the more reactive metal
60
Q

What is steel?

A
  • alloy of iron with some other elements
61
Q

What are ceramics made from and what are some examples?

A
  • made from clay
  • include bricks, porcelain etc.
62
Q

What is a composite material?

A
  • Composites are a mixture of substances that together provide properties suitable for a particular use
63
Q

What is a life cycle assessment?

A
  • Seeing the 4 stages of a material
    1. Extracting and processing of raw materials
    2. Manufacturing and packaging
    3. Use and operation during its lifetime
    4. Disposal at the end of its useful life

Chemistry (8 decks)

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