of alcohol burnt CONTROLLED VARIABLES: • The length of the wick coming from the spirit burner • Distance of the wick from the bottom of the aluminium can • Temperature change of the water in the aluminium can • Can used as calorimeter • Mass of water in calorimeter • The room temperature (environment) It is important that the controlled variables are all kept the same because it makes the experiment more reliable and accurate. Ways to ensure that the controls are kept the same is to record
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In this experiment‚ a coffee cup calorimeter was used to measure the temperature readings of a neutralization reaction and magnesium oxide‚ MgO. Calorimetry is used to measure amounts of heat transferred to or from a substance.2 The difference of temperatures was used to calculate the heat energy given off by each sub-reaction. These values were solved by using Hess’s Law which determined the overall enthalpy changes of the neutralization reaction and MgO formation. Hess’s Law states that the heat
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experiment‚ we us naphthalene as a fuel in bomb calorimeter which naphthalene powder is turned to pellet using pellet press. The fuel is burnt at constant volume condition in a high pressure container (the bomb). The whole bomb‚ pressurized with excess of oxygen. The mass of iron wire‚ ma =0.02g. The mass of naphthalene pellet with iron wire‚ mb =0.38g. The bomb is submerged in 850g of water and the initial temperature of calorimeter state temperature of calorimeter water before burning the fuel‚ Ti is
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procedures require the use of a calorimeter‚ which are of two types: a bomb calorimeter and a coffee cup calorimeter. Calorimeters are simply devices used to measure the amount of heat gained or lost in a system. Although this is not completely true‚ they are treated as isolated systems. A simple coffee-cup calorimeter can be constructed using two Styrofoam cups nested inside each other. The Styrofoam prevents heat loss to the surroundings‚ which makes it an ideal calorimeter.
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Discussions and Scientific Explanations The first goal of this project was to first construct a calorimeter. The second goal was to measure the heat capacity of the constructed calorimeter. The third and fourth goal was to determine what reactions were to be investigated and what variations of the reactions would be studied. The two requirements that were kept in mind while creating the calorimeter were that it should be a good insulator‚ meaning that it does not allow for the transfer of heat
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substance within the system”. Apparatus: Two (2) similar Calorimeters: a Thermometer: a Measuring Cylinder: a Bunsen burner: a Tripod: an Asbestos Gauze Cork Mat. Procedure: * The tripod and Bunsen burner were set up as shown in fig. 1 * Using the measuring cylinder 50gm of water was measured and poured into (1) one calorimeter labeled A‚ and 100gm was also measured and poured into the other calorimeter labeled B. * The calorimeter containing the 50gm of water was set on the cork mat
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(Fig-1)- Parr 6300 Bomb Calorimeter to calculate Gross Calorific value • A very programmed calorimeter to free the client from the manual operations required for normal calorimeters and minimize administrator time required per test. • A fast calorimeter fit for performing up to 8 tests in 60 minutes. • A high accuracy calorimeter fit for surpassing the repeatability and reproducibility necessities of all global standard test strategies. A full high lighted calorimeter equipped for stand alone
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The purpose of this experiment is to find what design of calorimeter captured the most energy from a combusted chip. To find this‚ we tested each design‚ and calculated the amount of energy it captured from a baked potato chip. The two basic forms of energy are kinetic energy and potential energy. Kinetic energy is the energy of motion. A ball has kinetic energy when it flies through the air. The ball has the ability to do work in that it can act upon other objects with when it collides. Potential
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Data Analysis: 1. What was the temperature change for the water in the calorimeter (ΔTwater)? 3°C 2. What was the temperature change for the metal sample (ΔTmetal)? Assume the intial temperature of the metal was the same as the temperature of the water it was boiled in. 70°C 3. What was the specific heat of water in J/g°C? 4.186 J/g°C 4. Using the following equation‚ your answers to questions 1-3‚ and your data table‚ determine the specific heat of the metal sample you tested. 5
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Experiment B2‚ Heats of Combustion – The Bomb Calorimeter. Objectives: To calibrate a bomb calorimeter by the combustion of benzoic acid. Then to use the calibrated calorimeter to measure the heat of combustion of naphthalene and calculate the heat of formation of naphthalene. Theory: q = C.ΔTBA C = q / ΔTBA Moles = mass / Mr ΔŪ = ΔU / moles ΔHoc‚298 = ΔŪoc‚298 + PDV = ΔŪoc‚298 + RTΔn C10H8 (s) + 12O2 (g) 10CO2 (g) + 4H2O (l) ΔHoc‚298 = - 1
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