If a company finds oil they need to ask the government if they can use.
There are three ways of getting oil out of the ground.
And they are
- fixed platform
- floating production facilities
- underwater production facilities
Separation of crude oil
The first thing we did was to boil the oil than as the small particles evaporate at a low temperature than they turned in to a liquid when they reach the condenser than they came out. As the molecules get longer they evaporate at a higher temperature and that goes on and on
Distillation in industries
As the oil goes in the tank the small molecules evaporate at a lower temperature so they goat the top of the tank but the large molecules evaporate at a high temperature so they go at the bottom of the tank.
The similarities and differences:
The similarities are
- They both use the same product. They use oil both of them
- The both have to go through the same process. To extract the oil in different fractions.
- Risk of getting fire they both have to be careful in case something happens so that it doesn’t blow up.
- They both use heat to boil the crude oil.
The differences are
- Scale of the equipment which is larger. They use more oil than laboratory.
- You have to make more products in industries. They make more products so that they can produce a good amount for all the other people.
- In industries you take all the fractions in the same time and in laboratory you take them 1 after the other. Because in industries you don’t have that much time to take one by one.
- The possible dangers are small in laboratory than in industries which they are much more dangerous. Because in industries because they got bigger equipment so there is a bigger danger.
Explanation:
These are the fractions of crude oil. The more carbons there are in the fractions the boiling range will be higher and they will have different uses. Than they will also have a higher boiling point and more viscous they will be less flammable and they will have a dark colour.
Volatility diagram
Gas has a low boiling point (high volatility) because gas molecules are easily separated. Bitumen has got a high boiling point and that’s because bitumen has molecules which are all together and they are hard to separate one from each other. The fractions in the middle will fit into this pattern.
How viscous it is
Gas is less viscous because all the molecules are separate so they move one by one. So that means when we pour the gas the molecules will drop one by one.
Bitumen is more viscous because when we pour the bitumen all the molecules are tangled together and they will pull each other.
And the fractions in the middle will fit into the pattern.
How flammable it is
Gas is more flammable because all the molecules are separated and each one of them has a bit of oxygen to help it burn.
Bitumen is less flammable because all the particles are together and they are hard to burn and they don’t have that much oxygen to help them burn. Only the particles at the end of the hydrocarbon chain will be able to react.
And the fractions in the middle will fit into the patterns.
Explanation of the colour
Gas has a light colour because the molecules are separated so it’s easy to see through.
Bitumen has a very dark colour because atoms and molecules are all together and it’s very hard to see through so that’s why it has a dark colour.
The other fractions in the middle will fit into the patterns.
Aim: To know how they are formed? To understand the difference between them?
Introduction: Alkanes and alkenes are two types of chemical they belong into two different groups which will be formed in different ways. Alkane A chemical composed of a straight chain of carbon atoms bonded on all sides by hydrogen atoms and containing no double bonds between carbon atoms. The simplest alkane is methane. Alkene A chemical composed of a straight chain of carbon and hydrogen atoms containing at least one double bond between carbon atoms. The simplest alkene is ethene (also known as ethylene) .Alkenes is highly flammable and burn readily in air, forming carbon dioxide and water.
Alkanes
- Functional group is the single C - C bond.
-
General formula CnH2n+2.
- They are relatively unreactive due to a strong single covalent bond.
- They are extensively used as fuels.
- Names end in -ane.
Alkenes
- Functional group is the double C = C bond.
-
General formula CnH2n.
- They are relatively reactive due to a weak double bond.
- They are extensively used as fuels, and as base for polymer manufacture.
- Names end in -ene.
Equipment:
- Test tubes
- Delivery tube
- Trough
- Bunsen burner
- Paraffin
- Glass wool
- Lime stone
Method: To do my experiment I used a few equipment. The first thing that I took was two test tubes and a delivery tube than I took a bit of glass wool and added a bit of paraffin and I put that into the one of the test-tube and and added a few crystal stones into the same test-tube. Than I put the delivery tube on than I took a Bunsen burner and lighted it up so that I can heat the test tube to get the gas and I also took a trough with water so that I can put the empty test tube on the water with the delivery tube inside the empty test-tube so that I can get all the gas that was produced in there and the gas produce was hydrogen.
The differences between alkanes and alkenes:
Alkanes are a family of saturated hydrocarbons potassium and sodium in group 1 of the periodic table; they react with water to produce hydrogen and alkalie solution CnH2n+2
Alkenes are a family unsaturated hydrocarbon compounds, including ethene and propene, with the general formula CnH 2n
Conclusion: In this experiment we used alkane and alkene to produce hydrogen the way that we did this was to heat the alkane and alkene so that they can speed the reaction and to make a chain compound which will produce hydrogen. Alkane and alkene are used in labs to make chemical reaction and its also used in polymerization, proteins, gasoline, waxes etc.We were certain what the gas was but if we want to find out we can do a pop test to make sure that it is the right gas produced.
Evaluation: If I had another chance to do this experiment again I will do it in a laboratory and I will use more equipment to do it and also do the test a few times so that I can make sure that I did it right.
Investigating fuels
Aim: To investigate the heat output of different at the molecules level. So will release different hydrocarbon fuels and to see which gave the most.
Hypothesis: The fuels are constructed differently at a molecules level. So will release different amounts of energy during combustion.
Hydrogen+ Oxygen→Carbon dioxide+ water+ energy
Equipment:
Diagram:
Safety:
Broken glass→ we walked and also got the equipment easily so that we can’t break any thing.
Eye damage→ we used goggles to protect our eyes.
Fumes→ we turned on the fans
Method:
- We seat up the apparatuses as in the diagram.
- We measured 5cm between the burner and the boiling tube.
-
We also measured 5cm³ of water into the boiling tube.
- Then we took the start of the temperature.
- Then we lighted the burner and started the stop watch at the same time.
- After 1minute we took the new temperature and recorded.
- We repeated this procedure for all six experiments.
Results:
Energy=mass of water • specific heat capacity of water • change in temperature of water
E (J) = 1ml of water is 1gm• 4.2 • (end temperature- start temperature)
Heptane
E (J) =5• 4.2 • (51-23)
=5 • 4.2 • 28 = 588 (J) 1 minute
Hexane
E (J) = 5 • 4.2 • (96-22)
=5 • 4.2 • 74 = 1554 (J) 1 minute
Pentane
E (J) = 5 • 4.2 • (99-29)
= 5 • 4.2 • 70 =1365 (J) 1 minute
Paraffin
E (J) =5 • 4.2 (90-34)
=5 • 4.2• 65 = 1365 (J) 1 minute
Octane
E (J) = 5 • 4.2 (99-34)
=5 • 4.2 • 6 5 = 1365 (J) 1 minute
Decane
E (J) = 5 • 4.2 (70-29)
= 5 • 4.2 • 41 = 961 (J) 1 minute
Conclusion: I found out that hexane released the most energy. There is disagreement in the group because others found other fuels released more energy. We will work out which fuels should have released the most energy.
Heptane
Heptane + oxygen →carbon dioxide + water
C7H + 11O2 → 7+CO2+8H2O
4• C-C 347= 2082
16• H-C 413= 6608
11• O=O 498= 5478
= 14168
7• 2 C=O 805= 11270
8• 2 H-O 464 = 7424
= 18694
∆= 18694
14168
4526
Hexane
Hexane + oxygen → carbon dioxide + water
2C6H14 + 19O2 → 12CO2 + 14H2O
2 • 5 • C-C 347= 3470
19 • O=O 498 = 9462
2 • 14 H-C 413 = 11564
= 24496
12 • 2 C=O 805 = 19320
14 • H-O 464 = 12992
= 32312
∆= 32312
124496
7816
Pentane
Pentane + oxygen → carbon dioxide + water
C5H12 + 8O2 → 5CO2 + 6H2O
4 • C-C 347 = 1388
12 • H-C 413=4956
8 • O=O 498 =3984
10328
5 • 2 C=O 805= 8050
6 • 2 H-O 464= 5568
13618
∆ = 13618
10328
3290
Paraffin
Paraffin + oxygen → carbon dioxide + water
2 C12H26 + 37O2 → 24CO2 + 26 H2O
2 • 11 C-C 347 = 7634
2 • 26 H-C 413 = 21476
37 • O=O 498 = 18426
= 47536
26 • 2 C-C 805= 38640
26 • 2 H-O 464= 24128
= 62768
2C18H38 + 45O2 → 36CO2 + 18H2O
2 • 17 C-C 347 = 11798
2 • 38 H-C 413 = 31388
45 • O=O 498 = 22410
= 65596
36 • C=O 805 =57 960
18 • 2 H-O 464 = 16704
= 74664
∆ = 74664
65596
= 9068
Octane
Octane + oxygen → carbon dioxide + water
2C8H18 + 25O2 → 16 CO2 + 18 H2O
7 • 2 C-C 347 = 4858
18 • 2 C-H 413 =14868
25 • 0=0 498 = 12450
32176
16 • 2 C=O 805 = 25760
18 • 2 H-C 464 = 16704
= 42464
∆ = 42464
32176
= 10288
Decane
Decane + oxygen → carbon dioxide + water
2C10H22 + 31O2 → 20CO2 + 26H2O
9 • 2 C-C 347 = 6246
22 • 2 H-C 413 = 18172
31 • O=O 498 = 15438
= 39856
20 • 2 C=O 805 = 32200
22 • 2 H-O 464 = 20416
= 52616
∆ = 39856
52616
= 92472
Errors:
- Measuring the temperature
- Measuring the time
- The water volume
- Measuring the distance
- Loss of energy due to flame movement
Improvement:
- We could put a tin can covering and burner and the boiling tube so that we could have more energy.
- Report followed by averaging will reduce error significantly.
Environmental impact of fuels:
The advantage of using hydrocarbons fuels are
- Its very helpful for cars so they can move easy
- It helps us to produce electricity
- It gives us gas, coal, oil and nuclear they all very useful to us in many ways e.g. gas is very useful because we burned to cook, coal is used to produce electricity, oil is used in cars and many other places and the last one is nuclear we used that to produce electricity.
The disadvantages of hydrocarbon fuels
- They are very dangerous to the environmental because the can cause green house effects
- They can make acid rain
- And they can cause global worming
The advantage oil fuel in the cars is because it helps them to move easily it is cheap to buy we can move things faster and it is very useful to us in many ways. Oil flues are good because we can move them around countries and use them in machines or for burning.
The disadvantages are that the fuels when they burn they make gas and they go in the clouds so the form rain and the rain is acid rain which is bad for the environment the acid rain can causes loads of damages in some ways like killing plant animals and it also corrodes some of the rocks.
I think that we should use less hydrocarbons because the disadvantages that I got shows why they are more important and its not good using oil and fuels because the are dangerous to earths the make loads of pollution they causes global worming and we also make electricity but we can have different ways of making electricity we can use water, we can get it from wind mills etc. so I think hat we should stop using hydrocarbons.
What is Renewable Energy?
Renewable energy refers to energy resources that occur naturally and repeatedly in the environmental and can be harnessed for human benefit. Examples of renewable energy systems include solar, wind, and geothermal energy (getting energy from the heat in the earth). We also get renewable energy from trees and plants, rivers, and even garbage.
Renewable energy encompasses many different types of technology at different stages of development and commercialisation, from the burning of wood for heat in the residential sector (traditional and low-technology) to wind-generated electricity (widespread and technically proven) to processes such as biomass gasification for electricity generation (still under development although some plants are operating).
Glossary
- Biomass energy: Changing farming wastes, grasses, trees, bark, sawdust, and other things into energy by burning it, changing it to a gas, or converting it to a liquid fuel.
- Energy crops: Crops grown specifically for their fuel value, including food crops such as corn and sugarcane, and non-food crops such as poplar trees and switch grass.
- Fossil fuels: Energy sources formed by the decay of plants, dinosaurs, and other animals over millions of years; coal, oil, and natural gas are fossil fuels.
- Geothermal energy: Using the heat from the earth to produce power.
- Hydropower: Using the energy in flowing water to make electricity.
- Municipal solid waste: Using trash or garbage to produce energy by burning it or by capturing the gasses it gives off and using them as fuel.
- Non-renewable fuels: Fuels that cannot be easily made or "renewed." We can use up non-renewable fuels. Oil, natural gas, and coal are non-renewable fuels.
- Passive solar heater: A solar water-heating or space-heating system that moves heated air or water without using pumps or fans.
- Passive solar home: A house that uses a room or another part of the building as a solar collector.
- Photovoltaic energy: A type of solar energy that converts sunshine into electricity.
- Renewable energy: Types of energy that are "renewed" as we use them; solar, wind, and geothermal energy are forms of renewable energy.
- Solar collectors: Boxes, frames, or rooms that trap the sun's rays to produce heat.
- Solar energy: Energy from the sun. The heat that builds up in your car when it is parked in the sun is an example of solar energy.
- Solar heating: Using the sun's energy to heat our homes and water.
- Sunspace: A room that faces south or a small structure attached to the south side of a house.
- Wind power: Using the wind to produce electricity by turning blades on a wind turbine.
- Wind power plant: A group of wind turbines interconnected to a common utility system.
Making Nylon
To do the experiment for making nylon we used two types of chemicals (1, 6-Diamino hexane 5% aquaes) and (Adipoyl chlorine% cyclohexane) we poured the first chemical in the beaker than we poured the other 1 in so that it floats at the top of the other chemical. They will mix the hydrocarbons together. So we mixed the two monomers to make the polymer which will be in the middle of the two chemicals so we used a forceps to take out the polymer. So that how we made polymers in the laboratory. The polymer we made was nylon.
Polymer: A substance made of many repeating chemical units or molecules. The term polymer is often used in place of plastic, rubber or elastomer. A polymer is a natural or synthetic compound of high molecular weight composed of long chains of repeating units, each relatively light and simple. Polymers are extremely useful in the manufacturing industry. They can be used to create materials for clothing, such as nylon and lycra. Polymers can also be used for making tires and shoes. Everything from windshield wipers to airplane wing fairings can be made from engineered plastics and polymer composites (Reisinger). However, the applications do not stop there. Most recently, scientists have been conducting research on utilizing polymers to facilitate transdermal drug delivery. Polymers are "long molecular chains formed by the chemical bonding of many molecules of one or more types" (tenenbaum). They compose many different materials and can be found throughout everyday life. Polymers come in shapes of many forms, including plastic, rubber, and synthetic fibres among many others.
Polymers can be used to create artificial skin that can facilitate the healing of wounds, especially for burn-victims.
Chemicals:
- 1, 6-Diamino hexane 5% aquaes.
- Adipoyl chlorine% cyclohexane
Equipment:
Safety:
- We wear goggles to protect our eyes from any gases.
- We used a forceps so that we can get the polymer in the middle of the two chemicals.
- We wear a monomer mask to protect our mouth from any gas which is dangerous to our body system.
- We use gloves so that we can protect are hands from the two chemicals or any acid.