The whole specification for IGCSE Chemistry has been completed. (Yay!)
Good Luck and happy studying.
Monday, 16 March 2015
Sunday, 15 March 2015
5d) Industrial manufacture of chemicals
Nitrogen from the air and hydrogen from either natural gas or from the cracking of hydrocarbons are used in the manufacture of ammonia
Haber Process:
Manufacture of ammonia
Uses of ammonia
- fertiliser
- nitric acid
- nylon fabric
Paper Two - Sulfuric acid
Raw materials used to manufacture it: sulfur and oxygen
Contact Process
Manufacture of sulfuric acid
Stage one: sulfur and oxygen --> sulfur dioxide
Stage two: sulfur dioxide and oxygen sulfur trioxide
Stage three: sulfur trioxide and conc sulfuric acid --> fuming sulfuric acid
Stage four: fuming sulfuric acid and water --> sulfuric acid
Conditions: 450C, 2 atmospheres of pressure and vanadiumn oxide (V2O5) catalyst
Uses of sulfuric acid:
- fertilisers
- detergents
- paints and pigments
- plastics
- paper and fibres
Electrolysis of Brine
Ions present: Na+ Cl- H+ OH-
Ion attraction to electrode:
Anode (+) Cl- OH-
Cathode (-) Na+ H+
Actual products: at cathode is hydrogen due to the reactivity series; lower reacting one forms out of possible products
at anode chlorine because if you have a halideion (group 7 ion) then the halogen will from, if not the oxygen will
Half Equations:
Cathode - 2H+ + 2e- --> H2
Anode - 2Cl- --> Cl2 + 2e-
Useful products
Haber Process:
Manufacture of ammonia
Uses of ammonia
- fertiliser
- nitric acid
- nylon fabric
Paper Two - Sulfuric acid
Raw materials used to manufacture it: sulfur and oxygen
Contact Process
Manufacture of sulfuric acid
Stage one: sulfur and oxygen --> sulfur dioxide
Stage two: sulfur dioxide and oxygen sulfur trioxide
Stage three: sulfur trioxide and conc sulfuric acid --> fuming sulfuric acid
Stage four: fuming sulfuric acid and water --> sulfuric acid
Conditions: 450C, 2 atmospheres of pressure and vanadiumn oxide (V2O5) catalyst
Uses of sulfuric acid:
- fertilisers
- detergents
- paints and pigments
- plastics
- paper and fibres
Electrolysis of Brine
Ions present: Na+ Cl- H+ OH-
Ion attraction to electrode:
Anode (+) Cl- OH-
Cathode (-) Na+ H+
Actual products: at cathode is hydrogen due to the reactivity series; lower reacting one forms out of possible products
at anode chlorine because if you have a halideion (group 7 ion) then the halogen will from, if not the oxygen will
Half Equations:
Cathode - 2H+ + 2e- --> H2
Anode - 2Cl- --> Cl2 + 2e-
Useful products
- Chlorine: sterilise water supplies and also used to make bleach and HCl
- Hydrogen: used in the haber process and changes oil into fat to make margarine
- Sodium Hydroxide: used to make soap, bleach and paper pulp
5c) Synthetic Polymers
A Monomer is a single molecule that join together to make a polymer
Polymers are long chain molecules made from monomers
Uses of polymers:
Poly(ethene)- plastic bags and bottles
Poly(propene)- crates and ropes
Poly(chloroethene)- water pipes and insulation on electricity cables
Disposal of addition polymers:
They are non-biodegradable because of their strong single bonds- inert
Some compounds are toxic if inhaled
They have to be put in land fills which occupy a lot of land in the UK, they can also be recycled or incinerated
Made from two different monomers and have atoms other than C (carbon) in main chain. These polymers also form small molecule as well as a polymer, usually H2O or HCl.
Polymers are long chain molecules made from monomers
Addition Polymers:
Uses of polymers:
Poly(ethene)- plastic bags and bottles
Poly(propene)- crates and ropes
Poly(chloroethene)- water pipes and insulation on electricity cables
Disposal of addition polymers:
They are non-biodegradable because of their strong single bonds- inert
Some compounds are toxic if inhaled
They have to be put in land fills which occupy a lot of land in the UK, they can also be recycled or incinerated
Paper Two- Condensation Polymers:
Made from two different monomers and have atoms other than C (carbon) in main chain. These polymers also form small molecule as well as a polymer, usually H2O or HCl.
Saturday, 14 March 2015
5b) Crude Oil
Crude Oil is a dark, smelly liquid which is a mixture of lots of different chemical compounds. A mixture contains two or more elements/ compounds that aren't chemically bond together.
Fractional Distillation:
-separates liquids with different boiling points
Incomplete combustion can produce carbon monoxide which is dangerous because it reduces the capacity of the blood to produce oxygen.
Fractional Distillation:
-separates liquids with different boiling points
- Oil heated as it enters fractioning column
- Chemicals in oil evaporate
- Those with lowest boiling points evaporate first
- They then condense to liquids
- Lowest boiling point chemicals move further up the fractioning column
- Liquid fractions drained off the column for use
Fraction | Boiling Range | Viscosity | Use | Chain length |
---|---|---|---|---|
Refinery gases
|
lowest
|
lowest
|
bottled gases
|
Shortest
C1 - C4
|
Gasoline
|
Petrol for cars
|
C5 - C9
|
||
Kerosine
|
Jet fuel
|
C12 - C15
|
||
Diesel
|
Fuel for cars/lorries
|
C15 - C20
|
||
Fuel oil
|
Fuel for ships
|
C21 upwards
|
||
Bitumen
|
highest
|
highest
|
Road buildings/ roofs
|
Longest around
C30
|
Incomplete combustion can produce carbon monoxide which is dangerous because it reduces the capacity of the blood to produce oxygen.
Sulfur dioxide and nitrogen come from burning fuel. The sulfur dioxide comes from sulfur impurities in the fossil fuels. Nitrogen oxides are created when the temperature is high enough for the nitrogen and oxygen in the air to react. This often happens in car engines. Nitrogen monoxide and nitrogen dioxide are included in nitrogen oxide.
Pollutants:
Acid rain is caused by sulfur dioxide and nitrogen oxides
When sulfur dioxide mixes with the clouds it forms dilute sulfuric acid, which is much more acidic
2SO2(g) + O2(g) + 2H2O ---> 2H2SO4(aq)
Nitrogen oxides can also form nitric acid in clouds, this rain is called acid rain.
Acid rain causes lakes to become acidic and many plants and animals die as a result and it also kills trees and damages limestone buildings and ruins stone statues.
Cracking
Converts long chain alkanes in the heavier freactions into shorter chains that are currently in more demand. Also as a result an alkene is also produced which is used to make polymers.
Conditions for cracking
-In industry vapourised hydrocarbons are passed over a powered catalyst at about 600C - 700C. Silica (SiO2) and alumina (Al2O3) are used as catalysts.
- heat the paraffin (or another alkane), after a few seconds move the bunsen burner to heat the catalyst. Alternate between the two until paraffin vapourises and catalyst glows red
- heated paraffin cracks as it passes over catalyst
- small alkanes collected at end of boiling tube and alkene gases travel down the delivery tube
- Alkenes are collected through water using a gas jar
5a) Extraction and Uses of metals
Methods of extraction are linked to the order of reactivity
Only metals that are less reactive than carbon can be extracted by a reduction reaction with carbon- this is done by heating the ore with carbon monoxide. This is because more reactive elements form compounds more readily.
Metals more reactive than carbon have to be extracted using electrolysis. It uses electricity to separate the metal from the other elements in the compound.
Aluminium extraction
Electroylsis is used to remove aluminium from its ore. A catalyst- Cryolite is used to lower the temperature and cost as Al2O3 has a very high boiling point of 2000C and so melting it would be very expensive. It is dissolved into molten cryolite which brings the temperature down to 900C, the electrodes are made of graphite which is a good conductor of electricity.
At the negative electrode (Cathode): Al3+ + 3e- --> Al
At the positive electrode (Anode): 2O2- --> O2 + 4e-
Uses of Aluminium
Only metals that are less reactive than carbon can be extracted by a reduction reaction with carbon- this is done by heating the ore with carbon monoxide. This is because more reactive elements form compounds more readily.
Metals more reactive than carbon have to be extracted using electrolysis. It uses electricity to separate the metal from the other elements in the compound.
Aluminium extraction
Electroylsis is used to remove aluminium from its ore. A catalyst- Cryolite is used to lower the temperature and cost as Al2O3 has a very high boiling point of 2000C and so melting it would be very expensive. It is dissolved into molten cryolite which brings the temperature down to 900C, the electrodes are made of graphite which is a good conductor of electricity.
At the negative electrode (Cathode): Al3+ + 3e- --> Al
At the positive electrode (Anode): 2O2- --> O2 + 4e-
Extracting Iron:
(Blast Furnace)
Raw materials:
- Iron ore -----> iron
- Coke -----> almost pure carbon; reducing iron oxide to iron metal
- Limestone -----> take away impurities from slag
- Air ------> allows the coke to burn
Reducing Iron ore to Iron:
- Hot air blasted into the furnace -----> coke burns faster than normal. Raises to 1500C.
- Coke burns and produces carbon dioxide:
- Carbon and Oxygen ------> Carbon Dioxide
- C + O2 ------> CO2
- Carbon monoxide
- Carbon dioxide and Carbon -----> Carbon monoxide
- CO2 + C -----> 2CO
- Carbon monoxide then reduces the iron ore to iron
- Carbon monoxide + Iron(II) oxide ------> Carbon dioxide + Iron
- 3CO + Fe2O3 ------> 3CO2 + 2Fe
- Iron is molten at temperature also dense so goes to the bottom where it's tapped off
Removing impurities:
Slag forms as CaO from limestone reacts with rocks (SiO2)
CaCO3 -----> CaO + CO2
CaO + SiO2 ------> CaSiO3 (molten slag)
- Coolen to solid and used for:
- road building
- fertiliser
Properties of both Iron and Aluminium
Uses of Iron
- both dense and shiny
- have high melting points
- strong and hard to break
- are malleable
- good conductors of heat and electricity
Uses of Iron
- doesn't corrode so is useful for products that come in contact with water such as drinks cans
- Used in bicycle frames and aeroplanes when the weight has to be very specific
4d) Equilibria
Some reaction are reversible which means that they have the same rate backwards and forwards
That means that there is no overall change: reactants --> products products --> reactants
This can only take place in a CLOSED system or it would escape. Initially there are no products when you first start to mix the reactants. After a while there will be products; but still more reactants. With time the reactants go down and the products go up and we reach the SAME RATE, this is called DYNAMIC EQUILIBRIUM.
The position of equilibrium is not always at the half way point therefore there could be a position where there is more reactants than products.
Dehydration of hydrated copper (II) sulfate:
hydrated copper(II) sulfate + heat anhydrous copper(II) sulfate + water
Heat makes the reaction go forwards (endothermic), whilst cold water makes it go backwards (exothermic)
Effect of heat on ammonium chloride:
Factors which influence equilibrium:
That means that there is no overall change: reactants --> products products --> reactants
This can only take place in a CLOSED system or it would escape. Initially there are no products when you first start to mix the reactants. After a while there will be products; but still more reactants. With time the reactants go down and the products go up and we reach the SAME RATE, this is called DYNAMIC EQUILIBRIUM.
The position of equilibrium is not always at the half way point therefore there could be a position where there is more reactants than products.
Dehydration of hydrated copper (II) sulfate:
hydrated copper(II) sulfate + heat anhydrous copper(II) sulfate + water
Heat makes the reaction go forwards (endothermic), whilst cold water makes it go backwards (exothermic)
Effect of heat on ammonium chloride:
ammonium chlorideammonia + hydrogen chloride
Ammonium chloride decomposes when it is heated so the forward reaction is endothermic, whilst the backwards reaction is exothermic
Factors which influence equilibrium:
- Temperature increase
- moves the equilibrium to the right hand side, in the direction that produces the fewer molecules/moles of gas on the RHS
- Pressure increase
- moves equilibrium to the right hand side, moves into the direction that absorbs heat energy e.g. endothermic reactions
- Concentration
- Catalyst to get products or reactants faster
LHS RHS
A + B C + D
Tuesday, 10 March 2015
4c) Rates of Reaction
RATE - AMOUNT REACTION⁄TIME
Depends on four things:
Depends on four things:
- Temperature
- Concentration
- Catalyst
- Size of particles (Surface area)
The Collision Theory:
Higher Temperature: particles move faster, collide more often and with more force. If the temp. is high there will be enough energy to overcome Ea.
Higher Concentration: more particles in more conc., so they collide more frequently
Large surface area: smaller pieces increase sa, more area to work on, collisions more frequent
Catalyst: increase the number of successful collisions by lowering the Ea.
Activation energy or Ea is the amount of energy needed to start a reaction
(higher temp. increases reaction)
Higher Temperature: particles move faster, collide more often and with more force. If the temp. is high there will be enough energy to overcome Ea.
Higher Concentration: more particles in more conc., so they collide more frequently
Large surface area: smaller pieces increase sa, more area to work on, collisions more frequent
Catalyst: increase the number of successful collisions by lowering the Ea.
Activation energy or Ea is the amount of energy needed to start a reaction
(higher temp. increases reaction)
4b) Energetics
Exothermic reactions:
Energy is transferred from the reacting mixture to the surroundings and temperature of surroundings increases
Endothermic:
Energy is transferred from the surroundings to the reaction mixture and temperature of surroundings decreases
Copper cup experiment is a simple calorimetry experiment:
Paper Two - Molar Enthalpy:
Measure temperature change of the experiment
Then use this calculation - Energy, Q = mc∆T m= mass of surroundings (water or solution) ∆T = change in temp.
or
∆H = Q/n n = number of moles sign - exo and + endo
∆H is the change in heat energy
Q is measured in Joules
Simple Energy Level Diagram:
Exothermic
Endothermic
Ea or activation energy is needed to break or make bonds
Bonds:
Breaking bonds puts energy in - endothermic,
whilst making new bonds releases energy - exothermic
Paper Two - Using average bond energies to calculate the enthalpy change during a simple chemical equation:
You are given the reaction and table of data
Then with the information work out the broken bonds (A) and the bonds you make (B)
Then subtract them to get the ∆H
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