Testing Alcohol
Testing Alcohol Aim To find out if the number of carbon and hydrogen atoms in alcohol affect how well they burn. Apparatus Clamp stand, alcohol burners containing: methanol, ethanol and propanol, splints, goggles, heat mat, copper beaker, water, thermometer, scales, water. Method Put 100g of water in a copper beaker and put in a thermometer, record the temperature and attach to clamp stand. Weigh the alcohol burner containing methanol and record the result, place under the beaker. Light the alcohol burner and wait till the water has reached 10 c more than the starting temperature. Put out the alcohol burner and weigh again. Then record the temperature the water is currently at and re-light the alcohol burner heat for another 10 c and then reweigh the alcohol burner and record the result. Repeat this for 10, 20, 30 and 40 c above the starting temperature, record the result for all of them. Now repeat the entire experiment again but using ethanol, then propanol in the alcohol burner. Results METHANOL 0 c 20 c 30 c 40 c Start temp ( c) 24 24 24 24 End Temp ( c) 36 50 54 64 Change in temp ( c) 2 26 30 40 Start Weight (g) 217.8 64.1 75.34 216.53 End Weight (g) 216.53 59.82 72.46 213.51 Change in weight (g) .27 4.28 2.88 3.02 Ethanol 0 c 20 c 30 c 40 c Start temp ( c) 24 25 26 22 End temp ( c) 34 45 56 63 Change in temp (
Reaction of Alcohol Lab
Name: Teacher: Date: October 16, 2010 Purpose: To test the theories of how the molecular structure of an organic molecule affects its properties and determine the different isomers of butanol through comparison of their reactions with distilled water, Lucas Reagent and Potassium Permanganate. Materials: - Unknown butanol isomers A, B, C, D - Pipettes - Distilled water - Lucas Reagent (conc. HCl + ZnCl2) - Potassium Permanganate (KMnO4) - pH probe/ pH paper - Test tubes (4) - Test tube rack - Rubber stoppers (4) - Goggles - 10-mL measuring cylinder - 25-mL measuring cylinder Flowchart: Prediction: Distilled Water Lucas Reagent Distilled Water & KMnO4 n-butanol Lowest solubility; mixture should be heterogeneous Takes much longer than 5min to turn cloudy Colour changes; pH should turn acidic, since it becomes an aldehyde and then a carboxylic acid i-butanol 2nd lowest solubility; mixture should be heterogeneous Takes much longer than 5min to turn cloudy Colour changes; pH should turn acidic; since it becomes an aldehyde and then a carboxylic acid s-butanol 2nd highest solubility; mixture should be heterogeneous Turns cloudy after ~5min Colour changes; pH should remain neutral, since it becomes a ketone t-butanol Highest solubility; mixture should be homogeneous Forms precipitate and turns cloudy immediately No colour change, since it
Burning Fuels Coursework
0/10/06 Chemistry Coursework In my chemistry coursework I will be investigating the amount of thermal energy different fuels will provide when burnt. My project brief is to "Examine alternative fuels for a power station that has until recently burnt coal. The fuel that gives the best value for money ratio will be the next one used in the power station." The costs of the fuels are: Fuel Cost in £ per kg. Methanol 5.10 Ethanol 7.20 Propan-1-ol 7.10 Butan-1-ol 6.20 Pentan-1-ol 16.90 Bond Energy Calculations The bond energy of a molecule is the energy released after it has reached the 'barrier' - the input energy needed for the bonds to break. Different bonds release different amounts of energy. The bond energy of all the fuels listed above needs to be calculated so that I can work out how much heat energy each fuel should theoretically produce when burnt, and then apply it to a formula to work out how cost effective that particular fuel is. Working out KJ/£ Methanol 6.81 KJ/g £5.10 per kg =0.00510 per gram 6.81 0.00510 = 3,296.08 KJ/£ Ethanol 22.51 KJ/g £7.20 per kg =0.00720 per gram 22.51 0.00720 = 3,126.39 KJ/£ Propan-1-ol 25.57 KJ/g £7.10 per kg =0.00710 per gram 25.57 0.00710 = 3601.41 KJ/£ Butan-1-ol 27.10 KJ/g £6.20 per kg =0.00620 per gram 27.10 0.00620 = 4,370.97 KJ/£ From my KJ/£ equations the
Experiment to investigate the heat of combustion of alcohols.
Chemistry AT1 - Experiment to investigate the heat of combustion of alcohols. Introduction. The heat of combustion of alcohols is the change in kJ/mol when 1 mole of the alcohol is burnt in excess oxygen (O2). I will be investigating 6 alcohols, using predictions and a practical to guide me through this experiment and form an overall conclusion. Using formulas and calculations, I can show how much energy is released from these substances, and work out their heat of combustion. From the homologous series of alcohols using the general formula of CnH2n+1OH, I have chosen 6 alcohols, giving the Mr for calculation purposes later on: Mr * Methanol - CH3OH 32 * Ethanol - C2H5OH 46 * Propanol - C3H7OH 60 * Butanol - C4H9OH 74 * Pentanol - C5H11OH 88 * Hexanol - C6H13OH 102 The reactants will produce the products of carbon dioxide and water (CO2): Alcohol + Oxygen Carbon Dioxide + Water I.E: C2 H5 OH + 3O2 2CO2 + 3H2O Apparatus List/Safety Precautions. * Tin can - For holding the water * 200 cm3 water - being heated by burning the alcohol. * Thermometer - measuring temperature accurately. * Heat-Proof Mat - keeping heat loss to minimum and safety against fires. * Spirit Burners - hold the alcohol that is going to be burnt. * Clamp Stand - hold the tin can in place. * Measuring Cylinders - Measure the amount of water accurately. *
Heat Energy Experiment Aim: To measure the heat energy released in a burning fuel.
Heat Energy Experiment Aim: To measure the heat energy released in a burning fuel. Diagram: Method: * The apparatus was set as shown in the diagram. * 20ml of water were measured. * The initial temperature of the water was measured as well as the distance from the tile to the bottom of the test tube. * The mass of the watch glass with and without the fuel was measured. * The fuel was lighted with a lighted splint and left to burn until it ends. * The mass of the watch glass was then re-measured. * The final temperature of the water was recorded. For safety reasons a heat-proof tile was placed under the watch glass and goggles were used. The fuel was lighted with a splint and not the Bunsen burner, and the experiment area was completely clear for space. For accuracy, the maximum temperature of the water was measured. The fuel was not left for a long time as the water would evaporate and the bottom of the test tube was cleaned in order not to interfere with the heating process. To make it a fair test, the time taken of different fuels to burn could be measured. If this happened, the apparatus should be properly washed, everything re-weighed and re-measured, and the thermometer left to cool. Results: (Averages) Ethanol Fire Lighter Distance from test tube to tile (cm) 2.5 cm 2.5 cm Initial temperature (ºC) 4.5 ºC 7.5 ºC Final Temperature
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
Chemistry Gold
I am assigned to complete a science piece of coursework on Gold and alloying, to start my assignment I would like to start off with a question, 'What is Gold?' Gold is an element, a precious metal which is usually found in mines like pieces or nuggets and then extracted into a pure metal. I have found out that and going to explain the physical properties of gold. Alloys are a blend of mixture of metals, the alloys as part of gold are referred to as carats, with pure gold as 24 carat gold. Therefore each carat represents approximately 4.17% by weight of gold. For example, a piece of 9 carat jewellery contains 37.5% by weight of gold, pure gold is yellow which makes it alluring. Gold has many features, some of the features are that it is soft, shiny, malleable (to be able to bend, which describes a metal that can be sharped without breaking), ductile (malleable enough to be worked: able to be drawn out into wire or hammered into very thin sheets. The most prominent use of gold is in jewellery (an item of adornment). Its other uses are, currency, computer chips, store of value, sculpture (gold plated items). The Properties of Pure Gold Pure gold which is 24 carat the most expensive because it is the most purest and has the least amount of other metals, and is actually bought for jewellery, the colour is yellow which also makes it charisma, this type of gold is the softest and
