Medical Cold Packs- Thermochemistry Experiment 2.1 Purpose: To use calorimetry to determine the enthalpy of solution of an unknown salt‚ and then to use that value to identify the salt in the medical cold pack. Materials: See handout Procedure: 1. Acquire two styrofoam cups‚ and cut the top off one of them. 2. Add 80mL of water and record it’s initial temperature. 3. Place 10g of salt into the water and put second on top‚ creating a seal. 4. Record the temperature
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of a system and its surroundings to change due to absorption or release of heat. The change in temperature‚ ΔT‚ can be measured and used to calculate the heat absorbed or released by the reaction. Heat‚ Q‚ is then used to calculate the change in Enthalpy‚ ΔH. To obtain the temperature change it is necessary to measure the initial temperature of the system/surroundings and also to determine the final‚ maximum temperature after the reaction. The temperature at the time of mixing cannot be determined
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CH213. Physical Chemistry II. Final Exam Your Name: Your Student Number: 110 Normal Points + 10 Bonus Points If you get 110 points out of 120 points‚ you will get the full 40% assigned to the midterm exam. Your scores 1) 2) 3) 4) 5) 6) Total: out of 25 out of 20 out of 20 out of 15 out of 20 out of 20 out of 120 * All the problems are connected. In other words‚ to solve the problem‚ you may need the information and/or answers given in other problems. All necessary information is basically
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hydrogen peroxide. Therefore‚ we found the heat capacity of calorimeter. After that‚ the enthalpy of decomposition of hydrogen peroxide was calculated by finding the amount of heat lost by solution and the heat absorbed by the calorimeter. Then‚ the heat absorbed by the calorimeter was subtracted from the heat lost by the solution to determine the amount of heat absorbed by hydrogen peroxide. The enthalpy of decomposition of hydrogen peroxide obtained is -57.9kJ/mol. Finally‚ we would look at how
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Introduction All chemical changes are accompanied by change in energy and this energy is in form of heat. The energy change of a reaction that happens at constant pressure is defined as heat of reaction or enthalpy change and the symbol ∆H is used to denote the enthalpy change. The enthalpy change can be either endothermic or exothermic. In endothermic reaction‚ ∆H > 0‚ meaning heat is absorbed by the system from the surrounding. In exothermic reaction‚ ∆H < 0‚
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------------------------------------------------- ------------------------------------------------- Mapua Institute of Technology ------------------------------------------------- School of Mechanical and Manufacturing Engineering ------------------------------------------------- ------------------------------------------------- ------------------------------------------------- PHYSICAL STUDY NO.2 ------------------------------------------------- -------------------------------------------------
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this is by using a homemade calorimeter. The calorimeter used in this experiment is made up of a Styrofoam ball with a hole that can fit a test tube. The heat capacity of the styro-ball calorimeter is measured using a neutralization reaction of know enthalpy change. This heat capacity is then used to calculate the amount of heat absorbed or released by a chemical reaction. This will be used to measure the heat of reaction of different reaction systems such as neutralization reactions‚ displacement‚ precipitation
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Thermodynamics- Enthalpy of Reaction and Hess’s Law Objectives: 1. To calculate the heat of reaction of a given reaction using the concepts derived from Hess’s Law. Pre-lab Questions: 1. Define Heat of Reaction. The enthalpy change associated with the completion of a chemical reaction. 2. Define Specific Heat. The energy it takes to raise the temperature of 1 gram of a substance by one degree Celsius. 3. Calculate the heat of reaction assuming no heat is lost to the calorimeter. Use correct
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Reaction - Hess’s Law Return The foundation of the study of thermochemistry was laid by the chemist Germain Hess‚ who investigated heat in chemical reactions during the last century. One statement of the law that bears Hess’s name says: The enthalpy change for any reaction depends on the products and reactants and is independent of the pathway or the number of steps between the reactant and product. In this experiment‚ you will measure and compare the quantity of heat involved in three reactions
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Chem 16 Notes UPD Should only be a supplement to discussions Table of Contents* [A] Lecture [1] Thermodynamics [2]Energy [3]Enthalpy [4]Hess’s Law [5]Determining Enthalpy [6]Heat Capacity [7]Calorimetry [8] Entropy [9] Gibb’s Free Energy [10] Waves [11] Quantum Theory [12] Quantum Numbers [13] Electron Configuration [14] Periodic Table [15] Periodic Trends KSev [16] Chemical Bonding [17] Formal Charge [18] Resonance Structure [19] Bonds [20] VSEPR [22] Valence Bond Theory [22] Molecular Orbital
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