An Investigation into using Alcohol’s as Fuel Sources
An Investigation into using Alcohol's as Fuel Sources Aim The aim of this investigation is to compare the efficiency of a series of alcohols as fuels Experimental Details Alcohols are a closely related group of organic molecules that are capable of being used as fuel sources, for example spirit burners. One of the alcohols to be tested is ethanol which is made from fermented sugar. All alcohols belong to a family of chemicals whose general formula is C H + OH, with n as a whole number. When any fuel burns it releases heat energy into the surroundings within where it lies. Therefore it is known as an exothermic reaction as it releases heat energy to its surroundings. When alcohol burns it releases two products which are carbon dioxide and water. In order to burn an alcohol you need to supply it with some sort of heat energy, the heat energy then breaks up the reacting molecules into individual atoms. Once the fuel has burnt the atoms begin to recombine to form the products of the reaction, as they recombine, energy is given out. The four alcohols I will be testing are propanol, butanol, methanol, ethanol. In order to find out which is most efficient I will need to find out the amount of energy that is burnt. The amount of energy that is theoretically released can be calculated when a fuel burns in sufficient oxygen to produce carbon dioxide and water as they are the
I am going to investigate how and why the enthalpy change is affected by the molecular structure of the alcohols under conditions, which I have stated under 'Plan' below.
Comparing the enthalpy changes of combustion of different alcohols Introduction I am going to investigate how and why the enthalpy change is affected by the molecular structure of the alcohols under conditions, which I have stated under 'Plan' below. Sources I have used the following sources in aid of devising my plan: * My lecture notes. * Salters Advanced Chemistry: Chemical Storylines * 'Enthalpy' coursework form www.essaybank.co.uk Equipment I will use the following equipment: * Copper calorimeter * Thermometer * Stand * Boss * Clamp * 200 cm³ measuring cylinder * Electronic balance * Bunsen burner * 2 Mats * 5 Splinters The above equipment are needed because the stand, boss and clamp will support and hold the metal calorimeter containing 200cm³ water, which it will be heated up by the burning alcohol underneath. The thermometer is used to measure temperature before and after the experiment and the electronic balance is used to weigh the alcohol before and after the experiment. Two mats will be used to keep heat loss, by heating the environment, to a minimum The Bunsen burner is used to light the splinter, which in turn will set alight the alcohol. Water level will be the same for each of the alcohols combusted. All of procedures are to be carried out just to make the experiment fair. Materials Only the following straight-chained alcohols will be
Find out which of five chosen fuels; Ethanol, Propan-1-ol, Butan-1-ol, Hexan-1-ol and Octan-1-ol gives out the most heat energy.
An experiment involving five fuels, to see which fuels contain most energy. Aim: To find out which of five chosen fuels; Ethanol, Propan-1-ol, Butan-1-ol, Hexan-1-ol and Octan-1-ol gives out the most heat energy. Introduction: A chemical bond is an attraction between atoms brought about by a sharing of electrons between to atoms or a complete transfer of electrons. There are three types of chemical bonds: Ionic, Covalent and Polar covalent. In addition chemists often recognize another type of bond called a hydrogen bond. Ionic bonds arise from elements with low electro negativity (almost empty outer shells) reacting with elements with high electro negativity (mostly full outer shells). In this case there is a complete transfer of electrons. Covalent bonds involve a complete sharing of electrons and occur most commonly between atoms that have partially filled outer shells or energy levels. Thus if the atoms are similar in negativity then the electrons will be shared. These bonds are in between covalent and ionic bonds in that the atoms share electrons but the electrons spend more of their time around on atom versus the others in the compound. This type of bond occurs when the atoms involved differ greatly in electro negativity. Prediction: I predict that the more energy given out, the higher the number of moles. Method: Equipment: * * Ethanol in fuel burner
To what extent can the audience sympathise with Hamlet?
indecision and his fretting over several different ideas at one time. Correspondingly Samuel Coleridge stated 'Saw in the prince a man whose intellectual energy and alertness understandably makes action impossible', both of these critics incorporating the idea that the audience is manipulated to sympathise with Hamlet as Shakespeare portrays him as a character who the audience can relate to. Another feature of the interpretation of the play is that, if the play were to be shown in Shakespeare's time the audience have a fair idea of what they are going to see. They know it's a revenge tragedy therefore somewhat limiting their reaction. However today's audience wouldn't be quite so well informed, consequently it is safe to deduct that the audience watching this play in modern times would be slightly more responsive towards Hamlet than in the time it was written. In act three, scene one the audience is placed with yet more motive for compassion for Hamlet. He is once again to be betrayed as possibly the love of his life is set up to deceive Hamlet. He never discloses any emotions or information to Horatio, seen as his only friend, and the love of his life betrays him. This secondary information is another reason Shakespeare includes to produce pathos, and it works just as he wishes. His views expressed to the audience before this are yet again questioning his inability to act.
Find out which fuel releases the most energy per gram.
Chemistry Plan Aim: To find out which fuel releases the most energy per gram. Scientific Theory: Heat is the transfer of energy between two objects due to a temperature. Heat is lost through the atmosphere because of combustion a process where a substance and oxygen or other elements combine to produce heat and light (fire). Combustion of alcohols produces water and carbon dioxide. Therefore the amount of heat which is not being used to heat the water is lost through the air. There are three types of heat: conduction, convection and radiation. There are a number of ways to control the heat lost, an example is taking tiles and surrounding the fire to decrease the area of the heat that can be lost so more heat is trapped to concentrate on the water. Another way to control the heat is to decrease the distance between the boiling tube and the container. The amount of energy released increases with the number of bonds present in the chemical substance or fuel. That is because each bond has a certain amount of energy stored in it therefore the more bonds the more energy is stored and more energy is released if these bonds break through combustion. Theoretical Values: Methanol CH OH 17000 J/g Ethanol C H OH 22000 J/g Propanol C H OH 25000 J/g Butanol C H OH 27000 J/g Hexane C H 35000 J/g Variables: The variables used in this experiment are: Volume of water, mass
Alcohols as fuels.
Alcohols as fuels Introduction: Alcohols, as most of us know burn quite well in air (they react with oxygen when heated in air). This means we could use alcohol as a fuel to produce energy, as the reaction with air is exothermic. What effect would using different alcohols as fuels have? We might expect to find that larger alcohol molecules could be burned to give out larger amounts of energy, as the structure contains more chains of molecules which can react with oxygen to release more energy. In this investigation, we shall test a range of alcohols to see how much energy each releases when combusted. Plan: We shall be investigating how different alcohols give out different amounts of energy when burnt in air. We shall be using methanol, ethanol, propanol, butanol and pentan-1-ol in this investigation. The best way to perform the experiment to find out how much energy is given out by each alcohol is to use alcohol burners. These are short glass cylinders which are sealed off at the top. They have a short piece of rope reaching from the bottom of inside the burner (where the alcohol would be) to a hole with a metal ring at the top of the burner. The metal ring can be taken off with the rope to refill the burner. We shall use these alcohol burners to heat up a metal beaker of 50ml of water by 40°C. We shall use a thermometer to measure this heat change. The flame of the
Are Congestion Zone a Good Idea?
Are Congestion Zones A Good Idea? By Katja Rackin In this report I will be finding out whether or not congestion zones are a good idea, using researched data, charts and tables to back up my ideas. The conclusion of this matter relies on how accurate and reliable the information is. Congestion Zones are used in hope that traffic gets reduced. The mayor of London has recently put congestion zones into place in hopes they will reduce traffic by 15%. The public has to pay £8 when entering congestion zones, however most money raised is used to improve public transport. Critics of the scheme however, say that it is unworkable and unfair. They also claim it will probably lead to more congestion as people try to avoid the charging areas. Central London has had a dramatic cut in traffic since the introduction of the congestion charge. 40 000 less people are driving through the zone each day as the number of cars entering the zone has dropped by 38%. Since the introduction of congestion charges average speeds have risen considerably. For example: average speeds have risen from 3mph to 7.4 mph and 9.8 mph was the highest average speed on the Embankment. This however is not recent research which could mean that it is slightly unreliable. More recent research therefore, suggests that traffic levels have built up to be closer to pre-charging levels since February 2004. As a result
Carbon chemistry
Introduction This experiment was conducted to find out the relative atomic mass of lithium. To ensure that the experiment was accurate I will use two different methods and if they are within 0.1 of each other I can be quite certain that my results are accurate. For the first method I will measure the volume of hydrogen when a known mass of lithium reacts with water. The second one will be a titration of the lithium hydroxide made in the first method. For this experiment I will be using * Lithium * 100cm3 distilled * 250cm3 measuring cylinder * 250cm3 conical flask * Stand * Plastic bowl Method: ) I will clean all equipment with distilled water. 2) I will set up my equipment properly so that the plastic bowl and cylinder have sufficient water in them. 3) I will clean the lithium to remove excess oil and cut it to the required mass. 4) I will place the lithium into water and shut the stopper as quickly as possible to prevent gas from escaping. 5) I will then weigh the lithium and record my results From knowing that 1 mole of gas occupies 24,000cm³ at room temperature and pressure I can deduce the amount of moles that I collected from the experiment Moles = 170 ÷ 24,000 = 0.00708 With these figures I can deduce the number of moles from lithium that reacted by using the ratio of lithium to hydrogen in the reaction 2Li (s) +2H2O (l) 2LiOH
GCSE Chemistry Coursework-Burning Fuels Investigation
GCSE CHEMISTRY COURSEWORK- BURNING FUELS INVESTIGATION CANDIDATE NO. 8218 - ANDRÉ SKEPPLE-GARRAWAY AIM: My aim is to measure the energy released by a series of alcohols. APPARATUS: Fuel, matches, stand, clamp, steel can, calibrated digital scales, thermometer (digital or alcohol), and stopwatch. METHOD: Fill can with 150cm³ of water. Then get a stand and the clamp and connect the clamp to the stand if it not already connected. Place the can filled with water and tighten it with the clamp. Then place a thermometer, either a digital on or an analogue one which uses alcohol and record the waters room temperature before the experiment. Then get the chosen fuel in its spirit burner container and measure its mass before the experiment on the digital scales and record it down in the table. Then open the cap of the fuel and light the wick of the burner with matches and heat the water with the flame for 3 minutes using the stopwatch and move the can slightly above the flame so that the flame is barely touching the steel can. Repeat with same fuel three times and then extinguish the flame by snuffing the flame putting the lid back on the spirit burner. Afterwards, measure the fuels mass on the scales again and record the waters temperature after the experiment. Record all the results in three different tables divided by the number of runs for each experiment. Once all the fuels
Alcohols Coursework
GCSE Chemistry - Alcohols Coursework Planning This investigation involves burning alcohol in the air. Key science- Chemistry by Eileen Ramsden says that " an alcohol is a series of organic, homologous compounds, with the general formula Cn H2n+1OH". The alcohol reacts with the oxygen in the air to form the products water and carbon dioxide: Cn H2n+1OH +(n+n/2)-1O2 ? nH2O + nCO2 The structure of the molecules in this reaction is: H H | | H - C - C - O- H + 3[O=O] ? 1/2[O=C=O] + 3[H-O-H] | | H H This reaction is exothermic, as heat is given out. This is because the amount reactant energy is more than the product energy the difference between this is ?H, therefore some energy has been given out in the form of heat.The energy is given out when forming the bonds between the new water and carbon dioxide molecules. This can be shown in an energy level diagram: Reaction co-ordinate ?H is the heat content, which is the enthalpy, which is negative in exothermic reactions as the diagram shows that energy is 'lost' as heat. Enthalpy is defined as the energy of reaction, or the heat energy associated with a chemical change. Chemical Principles By Master & Slowinski says that "For any reaction carried out directly at a constant pressure, the heat flow is exactly equal to the difference between enthalpy of products and that of the reactants", or: Qp = Hp - Hr = ?H Where Qp is the
