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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Bomb Calorimeter What is a Bomb Calorimeter? In calorimetry‚ a bomb calorimeter is a piece of equipment used to measure the heat fluctuation of a reaction’s system‚ the changes in physical properties and the thermal capacity. How does a Bomb Calorimeter works? A calorimeter is basically used for measuring the heat of fuels as it burns at a specific temperature in order to obtain the heat energy values. The samples of fuel used can either be solid or liquid but not gas. The calorimeters is estimated
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SPECTROPHOTOMETRIC DETERMINATION OF EQUILIBRIUM CONSTANT OF A REACTION UNIVERSITY OF THE PHILIPPINES‚ DILIMAN QUEZON CITY‚ PHILIPPINES August 2‚ 2013 ABSTRACT The objective of this experiment is to determine the equilibrium constant‚ denoted Keq‚ for the formation of [Fe(SCN)]2+ complex which is a product of the reaction between the ions Fe3+ and SCN-. In performing this experiment‚ solutions containing FeCl3 and KSCN‚ diluted in HCl‚ were measured for their absorbance using a UV-Vis
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The Enthalpy of Formation of Magnesium Carbonate By: Jessica Miller T.A: Thomas Lab Partner: Rebekah Melanson Thursday Lab Room 106 Chemistry 1001-A Due Date: Thursday February 3rd 2011 Abstract The purpose of this experiment was to determine the enthalpy of formation of magnesium carbonate in a lab setting. This was done using a calorimeter‚ which was calibrated by adding a known amount of both hot and cold water. Following the calibration of the calorimeter‚ HCl was placed into the empty calorimeter
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enzyme involves monitoring the change in absorbance of the reaction medium at 405 nm. Exergonic (i.e energy producing reactions) exhibit a negative free energy change. Sometimes these reactions occur spontaneously‚ but generally some energy must be supplied to initiate the reaction; in other word an energy barrier exists between the reactants and the products. The “energy barrier” represents the activation energy of a chemical reaction. In this practical the activation energy of hydrolysis
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Date Performed: January 10 & 15‚ 2013 Spectrophotometric Determination of the Equilibrium Constant of a Reaction R.J.V. Ortega and J.C.V. Gatdula Institute of Chemistry‚ College of Science University of the Philippines‚ Diliman‚ Quezon City‚ Philippines Received January 22‚ 2013 ------------------------------------------------- ------------------------------------------------- ------------------------------------------------- ABSTRACT -------------------------------------------------
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DATE PERFORMED: JULY 20‚ 2007 SPECTROPHOTOMETRIC DETERMINATION OF EQUILIBRIUM CONSTANT FOR A REACTION ABSTRACT UV-VIS spectrophotometry is one of the most widely-used methods for determining and identifying many inorganic species. During this experiment‚ this spectrophotometry was used to determine the equilibrium constant‚ Keq‚ of the Fe3+(aq)+SCN-(aq)↔ FeSCN2+(aq) reaction. By determining the amount of light absorbed‚ the concentration of the colored FeSCN2+ solution was also quantitatively
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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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gases‚ liquids‚ and solids in terms of the kinetic theory of matter. 8. Distinguish between endothermic and exothermic reactions. 9. Use thermochemical equations to describe energy changes in a chemical reaction. Readings and Assignments: Reading: 1. Principles of Heat Flow Section 8.1‚ pages 216-219 2. Measurement of Heat Flow Section 8.2‚ pages 219-222 3. Enthalpy Section 8.3‚ pages 222-223 4. Thermochemical Equations Sections 8.4‚ pages 223-226 Written Assignment 1. Principles
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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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