To measure and compare the enthalpy change of combustion for four different types of fuels by burning them and measuring the increase in the temperature of water in a calorimeter.
Chemistry Coursework Planning Aim: To measure and compare the enthalpy change of combustion for four different types of fuels by burning them and measuring the increase in the temperature of water in a calorimeter. From the increase in temperature of a known mass of water it is possible to calculate the enthalpy change of combustion (?Hc) for the fuels by the following formula Energy transfer = mass x Specific Heat Capacity x ?T joules Where ?T = the change in temperature in degrees Kelvin. The specific heat capacity of water is 4,2 J g-1 K-1 (Cambridge Chemistry 1). The specific heat capacity means the amount of energy required to raise 1 gram of water 1o C. The enthalpy change of combustion is when 1 mole of substance reacts completely with oxygen under standard conditions. Apparatus: > Small copper can which acts as a calorimeter, (base diameter 10cm). > 0-1100C thermometer > 100cm3 measuring cylinder > Spirit burners containing -methanol, ethanol, propan-1-ol and butan-1-ol. > Access to a weighing balance (2 d.p) > Draught shields Method: > Use 200 cm3 of cold water in a copper calorimeter and record its temperature. Measure the water volume using a burette because this as the smallest percentage error, of 0.175%. > Support the calorimeter over a spirit burner containing the fuel you are testing by using a clamp stand. Arrange a suitable position for
Propanol Investigation
Prediction & Hypothesis I predict that Propanol will produce the most heat on burning, as its energy out put is higher then any of the other Alcohols. I concluded by calculating the theoretical values of burning for each of the Alcohols. These were my calculations. > Methanol Word Equation Methanol + oxygen carbon dioxide + water Molecular Equation 2CH(3)OH + 3O(2) 2CO(2) + 4H(2)O Structural Equation H | H-C-O-H O=O H-O-H | O=C=O H + + H-O-H H O=O H-O-H | H-C-O-H O=C=O H-O-H | O=O H Bond Breaking Values Number Of Bonds to be Broken Type of Bond Relative amount of energy Needed per bond in kJ Total amount of energy needed in kJ 6 H-C 413 2478 2 C-O 358 716 2 O-H 464 928 3 O=O 498 494 Total amount of energy needed to break bonds in kJ +5616 Bond Creating Values Number Of Bonds to be Created Type of Bond Relative amount of energy Needed per bond in kJ Total amount of energy needed in kJ 4 O=C 805 3220 8 H-O 464 3712 Total amount of energy released Creating bonds in kJ - 6932 5616 6932 - -1316 The reaction is exothermic by. 1316 kJ > Ethanol Word Equation Ethanol + oxygen carbon dioxide + water Molecular Equation C (2) H (5) OH + 3O(2) 2CO(2)+ 3H(2) O Structural Equation H H | | H-C-C-O-H O=O H-O-H | | O=C=O H H + +
Investigation to Find the Relative Energy
Investigation to Find the Relative Energy Release of Five Alcohols: Ethanol, Methanol, Propanol, Butanol and Propanol Aim: In this experiment I will investigate to see which alcohol releases the most energy during combustion; Methanol, Ethanol, Propanol, Butanol or Pentanol. Hypothesis: I think that the alcohols with the longest carbon chains will release the most energy. This is because when a bond is broken energy is released. This means that the alcohols with longer chains and therefore more bonds will release more energy. This will mean they will heat the water quickest. This should mean that Pentanol will heat the water by the largest mount in 5 minutes. However, because of the longer hydrocarbon chains and therefore more bonds, Pentanol will also be the hardest to ignite, least volatile and least viscous. Despite the larger requirement for input of energy, the amount created by the breaking of bonds should increase by more which will mean that Pentanol will still release more energy than Methanol, Ethanol, Propanol and Butanol. To test this I have performed several calculations. By using figures for the amount of KJ/mol that the breaking of various bonds (O-O, C-H, O-H, C-C, C-O) release I have calculated the amount of energy that is needed to combust each of the alcohols. I have shown this information in a table below. Bond Energy released/required O-O +/-496
An Investigation to find out how and Why enthalpy change is affected By the molecular structure of alcohols
An Investigation to find out how and Why enthalpy change is affected By the molecular structure of alcohols The goal of this investigation is to ascertain the difference in enthalpy change of combustion for a variety of alcohols. From these differences, I will be able to deduce why and how enthalpy change is affected by different molecular structures. The enthalpy change of combustion of fuel is a measure of the energy transferred when one mole of fuel is completely combusted. To find out the enthalpy change of combustion for alcohols I am going to use the burning alcohol to heat a metal container filled with Water. Using the fact that Water (H2O) needs 4.2J of energy to raise the temperature of 1 gram of Water by 1 c. From prior Knowledge, I know that 1g of water is equal to 1ml of water. This investigation will have to be carried out in the delta H standard, which is completing the investigation in standard temperature(298K, or 25c), Standard pressure of one atmosphere and a standard concentration of 1 mol dm. To work out the enthalpy change you need the equation CM T. C is equal to the specific heating capacity of water (4.17Jg 1K 1). M is equal to the mass of water in grams. T is the temperature of water. For this investigation, I have chosen the following alcohols, Methanol, Ethanol, Propan-1-ol, Butan-1-ol and 2-Methylpropan-1-ol. I chose this range of
Is the kind of sugar determinative for the release of a higher measure of ethanol? If so, which sugar releases the most ethanol?
Yeast and fermentation: four different sugars Karlijn Hasaart en Esmée de Looff Summary On the occasion of the experiment which is performed by Slaa et al. (2009); Yeast and Fermentation: the optimal temperature, we performed a following experiment by ourselves with the inquiry question: Is the kind of sugar determinative for the release of a higher measure of ethanol? If so, which sugar releases the most ethanol? We researched the different productions of ethanol and carbon dioxide by using four different kind of sugars; glucose, cane sugar, fruit sugar and malt sugar. First of all we put the solutions of the different sugars with water and yeast by a temperature of 25 degrees (298 K) for about two days. And then we put all the solutions in a warmth bath of 37 degrees (310 K). After three days we came back and we were able to conclude something we didn't expect. Introduction Slaa et al. (2009) did their experiment based on the fact that oil resources will be exhausted. This knowledge stimulated Slaa et al.'s interest in one of mankind's oldest chemical processes: the production of bio-ethanol from sugars by fermentation. In stead of the temperature as a independent variable, we took the different kind of sugars as a independent variable. We used glucose, cane sugar, fruit sugar and malt sugar for our experiment. The molecular formulas of these sugars and their
Global Warming
Heads Up! Oceans Rising Faster Near Coasts April 26, 2004... According to Simon Holgate and Philip Woodworth of Proud man Oceanographic Laboratory, in Bidston , UK , satellite measurements of sea levels have revealed the sea seems to be rising faster near the coast than in mid-ocean. This is attributed of global warming in that, as water in the oceans expands as it warms up, and more is added as glaciers and ice caps melt. However, the satellite also reveals an unexpected phenomenon: during the same period, the water level within 100 kilometres of the coast rose faster, by an average of 3.7 millimetres a year. Holgate and Woodworth conjecture the oceans are behaving like water in a bathtub. If you splash in the bath, waves travel outwards and then run around the edges of the tub. This hypothesis was first proposed by Kirk Bryan of Princeton University and his colleagues in 1996, when they theorized what would happen when part of an ocean heats up: the water expands, creating "boundary" waves that hit the coast and then travel around the rim of the ocean basin for several years. This may not necessarily be bad news for people who live near the shore. The boundary waves could be caused by some relatively sudden event, such as a particularly warm year, in which case they will subside. However, if they are driven by an ongoing process of climate change, the difference
Describe, in terms of production of photochemical smog, what is meant by primary pollutants and secondary pollutants in the atmosphere, and list the main primary and secondary pollutants produced as a result of motor vehicles.
Chemistry Open Book 2003 Describe, in terms of production of photochemical smog, what is meant by primary pollutants and secondary pollutants in the atmosphere, and list the main primary and secondary pollutants produced as a result of motor vehicles The combustion of fossil fuels in vehicles releases incompletely burnt chemicals and oxidised species known as primary pollutants into the atmosphere. Many of the primary pollutants undergo further reaction under the influence of sunlight. The produces of these photochemical reactions are called secondary pollutants. Primary pollutants consist of oxides of nitrogen. In the atmosphere nitric acid, which is produced by high temperature combustion cylinders in engines, is oxidised to the brown gas nitrogen dioxide NO2, a major constituent to smog. Primary NOX (NO + NO2), CO Secondary: O3, NO2, H2O2, PAN (peroxyacetyl nitrate), partially oxidised VOCs HNO3 Describe how primary pollutants are formed in the combustion of the fuel in a coal-fired power station Coal-fired power stations have three main inputs, coal, cooling water and very pure water. The coal that is used contains compounds of nitrogen, formed from proteins contained in organisms. When the compounds are burnt they are oxidised to form what is called fuel NOx[1] N2(g) + O2 2NO(g) 2NO(g) + O2
Describe, in terms of production of photochemical smog, what is meant by primary pollutants and secondary pollutants in the atmosphere, and list the main primary and secondary pollutants produced as a result of motor vehicles.
Chemistry Open Book 2003 Describe, in terms of production of photochemical smog, what is meant by primary pollutants and secondary pollutants in the atmosphere, and list the main primary and secondary pollutants produced as a result of motor vehicles The combustion of fossil fuels in vehicles releases incompletely burnt chemicals and oxidised species known as primary pollutants into the atmosphere. The dangers they pose range from eye irritation to global warming. Many of the primary pollutants undergo further reaction under the influence of sunlight. The produces of these photochemical reactions are called secondary pollutants. Primary pollutants consist of oxides of nitrogen. In the atmosphere nitric acid, which is produced by high temperature combustion cylinders in engines, is oxidised to the brown gas nitrogen dioxide NO2, a major constituent to smog. N2(g) + O2 2NO(g) 2NO(g) + O2 2NO2(g) Describe how primary pollutants are formed in the combustion of the fuel in a coal-fired power station Describe and explain the most favourable conditions for forming photochemical smog, and how the high concentrations of tropospheric ozone are produced Describe the chemistry of the processes chosen as BPEOs at Longannet for minimising sulphur dioxide and NOx, emissions, and suggest why the Longannet management made
Alcohol Combustion Experiment
Planning In this investigation I will be burning alcohols to heat up a beaker of water. I will be burning five alcohols, methanol, ethanol, propanol, butanol and pentanol. The aim is to find out how much energy is produced when burning these alcohols. 'An alcohol is a series of organic homologous compounds, with the general formula Cn H n + 1OH´. Alcohols react with oxygen in the air to form water and carbon dioxide. The reaction that is involved in burning alcohols is exothermic because heat is given out. Form this reason the reactant energy is higher than that of the product. The energy is given out when forming the bonds between the new water and carbon dioxide molecules. The amount of energy produced by such exothermic reactions can be calculated by using the formula Mass of the substance x rise in temp x SHC( specific heat capacity). The specific heat capacity is the number of joules required to heat one gram of water by 1ºC. I chose to use water because it is safe, easily found, and has a reliable specific heat capacity of 4.2. The bond that are formed in an exothermic reaction can be of two types. The first could be ionic, where a metal is produced. Ionic bonding involves electrons transferring from one atom to the other consequently leaving an electrostatic force between them. The other form of bonding is covalent where atoms share electrons to complete their
Burning Alcohols.
Chemistry coursework Sarah Kennedy Burning Alcohols We are going to be doing an experiment that will show us how much heat energy is produced by burning an alcohol. The amount of heat given out when a mole of fuel burns is called heat combustion( H combustion). We will test how much energy is produced by calculating the heat given of from the alcohol burned by the spirit lamp. In this each experiment the variable is going to be the different alcohols used. I am going to have four different alcohols; Methanol, Propanol, Ethanol and Butanol. The outcome of this experiment will be the mass difference from the beginning to the end and the temperature change. From that we can find out the heat per mole given out for all of theses alcohols. Method: Safety is important whilst doing this experiment so hair should be tied back, overall and goggles should be worn during experiment and the surface where the experiment is taking place should be clear. The equipment needed for this experiment will be; a retort stand, clamp, boss, measuring cylinder, thermometer, glass beaker, heat proof mat, splint, spirit lamp with a lid, draught shield, boss and a balance. Light the spirit lamp and measure the size of the flame then record it. Extinguish the flame by putting the lid back onto the lamp. Weigh the lamp on a balance with its lid then record its mass. Then fill a beaker with
