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Distillation	Is used to separate the components in a mixture of liquid which have different boiling points. E.g A mixture of ethanol (b.p 78) and water (b.p 100)
Fractional Distillation	Used when the components in a mixture have very similar boiling points.
Fraction	Is a mixture of hydrocarbons of similar Carbon Chain length.
Crude oil	Mixture of many different hydrocarbons.
Hydrocarbons	Compounds made up of Hydrogen and Carbon only.
Crude oil seperation	Different fractions have different boiling points and this property is used to separate fractions from crude oil.
Fractional Distillation column	Image: 0f4559f1-1a0c-4a4b-88ab-7b2382a48d1e.JPG (image/JPG)
Alkanes	Saturated (Maximum possible hydrocarbons) Hydrocarbons (compounds of carbon and hydrogen) No Carbon-Carbon double bond General formula= CnH2n+2 Carbon makes 4 bonds Hydrogen makes 1 bond
General Alkanes	h Methane= CH4 h c h h Ethane=C2H6 Propane=C3H8 Butane=C4H10 Pentane=C5H12
Distillation Properties	Flammability Viscosity(Thickness) Size of Carbon Chains
Burning Fuels	Hydrocarbon + Oxygen -> Carbon Dioxide + Water Coal + Impurities of Sulphur + Oxygen -> CO2 +H2O + Sulphur Dioxide Hydrocarbon + Insufficient O2 -> Carbon Monoxide + H2O
Pollutants	CO2 = Global Warming Carbon Monoxide= Poisonous Sulphur Dioxide= Acid Rain Nitrogen oxide= Acid Rain + Triggers asthma Carbon Particulates(small particles of carbon)= Smog/smoke/fog -> poor visibility
Alternative fuels	Hydrogen Ethanol Biodiesel
Using Hydrogen as a fuel	Production= Electrolysis of water 2H2O -> 2H2 +O2 OR Using Methane= Methane + Steam-> Carbon monoxide + Hydrogen Burning hydrogen= H2+O2 -> H20
Advantages of using Hydrogen as a fuel	Only water vapours are produced when burnt.
Disadvantages of using Hydrogen as a fuel	Formation of Hydrogen produces a poisonous gas (Methane production). Electrolysis of water needs electricity. Can explode as it is highly flammable. H2 is a gas, so storage is a problem as it needs low temperature, but high pressure.
Using Ethanol as a fuel	An Alcohol. Production of ethanol= Glucose(sugarcane) ->(yeast and 37C) Ethanol +CO2 C6H12O6 -> C2H5OH +CO2
Advantages of using Ethanol as a fuel	Renewable Carbon neutral fuel.(?)
Disadvantages of using ethanol as a fuel	Burning Ethanol produces CO2. Quite flammable. Shortage of land-shortage of food crops-starvation.
Bio-diesel	A fuel produced from plant sources.
Production of bio-desiel	Image: b50a4e32-638b-450d-b25e-5bfe15611936 (image/jpg)
Combustion	Hydrocarbon + Oxygen -> Carbon dioxide + Water Hydrocarbon = (Insufficient) Oxygen -> Carbon monoxide + Water + Carbon Sulphur + Hydrocarbon + Oxygen -> Carbon dioxide + Sulphur dioxide + Water Nitrogen + Oxygen -> (High Temperature) Nitrogen oxide
(Catalytic) Cracking	The process where larger, less useful hydrocarbons are broken into smaller and more useful molecules, using heat and a catalyst. An example of Thermal Decompostion.
An example of Cracking	Octane -> Ethene + Hexane (Heated to 800C with AL2O3 or Aluminum oxide/Alumina) h h C8H18 -> C=C h h + C6H14
Definition of Catalyst	A substance which speeds up the reaction without being used up within the reaction.
Alkenes	Unsaturated Hydrocarbons Unsaturated means in the molecule there is at least ONE carbon-carbon double bond present e.g C=C
General Formula for Alkenes	CnH2n
Bromine Water and Alkenes/Alkanes	Bromine water starts of yellow/orange Bromine water stays the same colour in the presence of an ALKANE Bromine water goes colourless in the presence of an ALKENE.
Demand for ALKANES	Shorter alkanes are more in demand than longer alkanes because they are used as fuel/easier to ignite A fraction of crude oil that has more demand than what meets supply is petrol. One fraction of crude oil that is in greater supply than demand is fuel oil.
Products made from cracking	Alkanes= Fuels Alkenes= Plastics
Polymers	Plastics are long chained molecules (1000s of atoms) Long chained molecules are called polymers which are formed by joining small molecules called monomers. Formed when many monomers join together- reaction called addition polymerisation
Monomers	Small molecules At least ONE carbon-carbon double bond.
Polymer formula	h h n C=C h h -> (h h) (C=C) ( h h)
Polymer examples	Propene -> Polypropene Styrene -> Polystyrene Vinylchloride -> Polyvinylchloride
Designer Polymers	Polymers that have been designer for different uses.
Shape memory polymer	A polymer that changes shape as the temperature changes. Useful for braces.
Hydrogels	Polymers that work by when the sodium particulates are taken away, the polymer uncoils and the water molecules are attracted to the uncoiled chains. Useful for nappies
Dental polymers	Polymers that when UV light is shone on them, they paste together. Better than metal fillings as they don't conduct heat, and they paste together to make a solid filling. Useful for fillings
Polymer developments	1. Food packaging that changes colour when food goes off. 2. Anti-microbial chemicals in packaging to extend shelf life.
PTFE	Breathable fabric- allow water from sweat to escape. Work- three layers, outer, PTFE, inner. Outer layer gets wet. PTFE- small holes to allow water vapour through, but not water droplets.
Disposing of plastics	Burning polymers Burying plastics Exporting plastic Re-using plastic Reducing plastic Recycling plastic Bio-degradable plastic
Burning plastics	adv- can be used to generate electricity dis- plastics give off toxic fumes when burnt
Burying plastics	Does not biodegrade.
Exporting plastic	Places such as New York have run out of room in landfill- export out of the state to get rid off their plastic,- somewhere else has to deal with it.
Re-using plastic	adv- easy to do dis- most plastic is used for packaging, and thus a one off use.
Reducing plastic use	Some foods can be used to make packaging. Paper bags. Wrapping food in greaseproof paper rather than cling film.
Types of plastic (main types)	1.PETE poly(ethene)terephthalate 2. HDPE High density poly(ethene) 3. PVC Poly Vinyl Chloride 4. LDPE Low density poly(ethene) 5. PP Poly(propene) 6. PS Polysterene
Biodegradable plastics	Scientists use biotechnology to change genes in potatoes, so they make plastic instead of starch.
Ethanol	C2H5OH
Uses of ethanol	1. Biofuel 2. Alcoholic drinks 3. Hand gel, aftershave, perfumes (low boiling point) 4. Disinfectant in hospital hand gel
Making ethanol (Fermentation of carbohydrate)	Fermentation of plant source C6H12O6 ->(yeast) CO2 + C2H5OH 37C (35C-40C) Normal (low) pressure Yeast catalyst Absence of oxygen+water Batch process (stop/start-labour intensive) Slow reaction + impure ethanol Sustainable Carbon neutral
Making ethanol (Ethane + steam)	Crude oil CH2 = CH2 +H2O -> C2H5OH 300C 60-80 atm (pressure) Phosphoric acid as a catalyst Continuous process Fast reaction rate Pure ethanol Not sustainable Energy is needed and uses non renewable resources
Extraction of plant oils Crushing	1. Seeds/plant material is crushed. 2. Oil is removed via pressing. 3. Unrefined oil with impurities. 4. Impurities removed. 5. Refined oil obtained.
Extraction of plant oils Boiling	1. Plants put in boiling water. 2. Oil evaporates from plants. 3. Collected by condensing it. 4. Water and impurities removed for pure oil.
Types of oils	Saturated oils Monounsaturated oils Polyunsaturated oils
Saturated oils	Only carbon-carbon SINGLE bonds present NO carbon-carbon double bonds
Monounsaturated oils	Only ONE carbon-carbon DOUBLE bond present
Polyunsaturated oils	Many Carbon-Carbon DOUBLE bonds present. "Healthy" oil.
Detection of unsaturation	Bromine water- Yellow Br2 turns colourless Iodine water -Brown I2 water turns colourless n.b mor unsaturation in the molecules, the more Br2/I2 water will be needed.
Saturated oil/fat	Solid at room temperature High melting point Mainly present in animals Unhealthy
Unsaturated oil/fat	Liquid at room temperature (usually) Low boiling point Plant oils are mostly unsaturated Healthy
Hydrogenation/hardening of oil	Number of Carbon-Carbon double bonds are reduced by reacting vegetable oil with hydrogen in the presence of a catalyst. Useful- making margarine form sunflower oil and spreads.
Emulsions	Formed when droplets of one liquid (i.e oil) are suspended in another liquid (i.e water)
Water and oil	DO NOT MIX Water is polar, oil is nonpolar Water molecule- small Oil molecule- large
Immiscible	Two liquids that DO NOT MIX
Miscible	Two liquids that MIX
Emulsifier	The molecule that slows the time taken for the immiscible liquids to seperate
Formation of an emulsion Oil and water	Emulsifier's hydrophobic tail binds with oil, hydrophilic head binds with water. Charged droplets repel each other- spread apart in water. Small droplets collide + form bigger droplets. Mixture separates and two layers form. Emulsion with emulsifier takes longer to separate.
Earth's structure	asdfghjkl;

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