= 0.025kg ± 0.00001 Temperature change‚ T = 57.50 – 26.00 = 31.5C ± 0.1 Heat evolved‚Q = mHCLcwT = 0.025kg x 4200Jkg-1K-1x 31.5C = 3.3075 kJ H = -Q/1000n = -3.3075kJ/0.025 mol = -132.3 kJmol-1 Uncertainty of enthalpy change of reaction of H2 Part 1 The uncertainty for the reaction above is as follows:
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LH of steam (9H/100+M/100) II-1 CHEMICAL REACTIONS Combustion C + O2 = CO2 + 32‚790 kJ/kg of carbon‚ Heat of formation at 25C is 393.7 kJ/mol [Perry p-2-188] mCn Hm + (n +m/4)O2 = nCO2 + m/2 H2O + Q S + O2 = SO2 + 9260 kJ/kg of sulfur Calcination CaCO3 = CaO + CO2 – 1830 kJ/kg of CaCO3gCO3 = MgO + CO2 – 1183 kJ/kg of MgCO3. Sulfation CaO + SO2 + 1/2 O2 = CaSO4 + 15141 kJ/kg S. Basic Stoichiometry C + O2 = CO2 + q 1 kmol of carbon combines with 1
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ENGINEERING THERMODYNAMICS Dr. Tamer A. Tabet Course Code: KC1702 and Mechanical Eng. Programme‚ KM21102. SEMS-1-2011/2012 Lecture 6. Tue. 15 / 10/ 2012 Lecture Room DKP 10 Engineering Thermodynamics Lecture 6: Evaluating Properties Using the Ideal gas OUTLINE: Real gases‚ specific heats‚ internal energy‚ enthalpy In this section the ideal gas model is introduced. The ideal gas model has many applications in engineering practice and is frequently used in subsequent section
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figures. 11. Write a balanced chemical equation for the combustion of benzene‚ C6H6. 12. If the standard heat of combustion of benzene is –3271 kJ/mol‚ [(CO2(g)] = –394 kJ/mol‚ and [H2O(l)] = –286 kJ/mol‚ calculate the standard heat of formation of benzene. Report your answer to the correct number of significant figures. 13. If a gas sample absorbs 59 kJ of heat
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½O2(g) ( H2O(l) + 285.8 kJ 2. Indicate the enthalpy of reaction as a separate expression beside the chemical equation. H2(g) + ½O2(g) ( H2O(l) ΔHorxn= -285.8 kJ For exothermic reactions‚ ΔHorxn values are always negative. 3. Represent the enthalpy of reaction on an enthalpy level diagram. Representing Endothermic Reactions 1. Using a thermochemical equation where the enthalpy of the reaction appears on the reactant side of the reaction. MgCO3(s) + 117.3 kJ ( MgO(s) + CO2(g)
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Energy in food lab report Aim: How much energy there is in food. Hypothesis: If I work out how much the water temperature has risen by burning food underneath water‚ the mass of the water and the mass of food I can work out how much energy was in the food. Introduction: This experiment is about how much energy there is in food. There are a few different types of energy‚ the one we are looking at is chemical energy. Some other types of energy are: thermal energy which is heat‚ magnetic energy which
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Thermochemistry Saxon Evans & Zac Taylor Dr. Nachman 2/08/2011 Abstract: Using the chemical equation we can study the reaction taking place between magnesium metal and sulfuric acid in solution. The = for the reaction of sulfuric acid and magnesium metal. Introduction This report demonstrates calorimetry‚ or the technique of measuring heat effects in the surroundings. In order to make sure that there is no temperature change‚ or that it is an isothermal heat transfer‚ it is kept
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Determining the enthalpy change for the thermal decomposition of potassium hydrogen carbonate into potassium carbonate. Controlled Variables: 1. Volume of HCl ± 0.5 cm3 (± 2%) 2. Concentration of HCl‚ 3. Same mass of K2CO3 and KHCO3 within specified ranges of 2.5 – 3.0g and 3.25 – 3.75g respectively 4. Same calorimeter used i.e. polystyrene cup is used in this experiment 5. Same thermometer will be used ± 0.10K 6. Same source of K2CO3‚ KHCO3 and HCl Raw Data Results: The raw
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combustion of naphthalene was experimentally determined to be -5030.44 ± 78.98 kJ/mol which was a 2.5% error from the literature value of -5160 ± 20 kJ/mol.2 The theoretical enthalpy of combustion of solid naphthalene was calculated to be -6862.68 kJ/mol using bond energies for the gaseous molecules‚ the heat of vaporization of liquid water and the literature value of the heat of sublimation of naphthalene‚ which was 72 ± 4 kJ/mol.2 The absolute value of the difference between the theoretical heat of
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Introduction Enthalpy change‚ ΔH‚ is defined as the heat output of a system as it goes through a reaction under constant pressure. It is an important aspect of thermochemistry‚ which is the study of energy changes during a chemical or physical reaction . When we calculate enthalpy change‚ we always assume that the pressure is constant. We are able to calculate enthalpy change numerous ways‚ notably by the increase in heat‚ Q‚ given by an exothermic reaction or the heat absorbed by an endothermic
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