Title Page: Module Code: FC 511 2T Module Title: Skills for study Tutor Name: Emma Duffy Assessment title: Formative Lab Report: Enthalpy of Combustion of Butanol Student ID Number: 201233920 Date of submission: 6/3/2017 Past tense recapping what you did in the experiment Present tense explain theory and compare theory THINGS TO IMPROVE : Reference Introduction Discussion Avoid Plagiarism Table of Contents Introduction P.3 Aim Materials
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Lab 5 DECOMPOSITION (Nov 2‚ 2011) Introduction: Decomposition is the breakdown of organic material into its smaller molecules and elements. (This term is generally considered as a biotic process but one may find it also used to describe an abiotic process‚ e.g.‚ due to weathering.) The decomposing organisms may use the release of elements for nutrients and by breaking apart the carbon-carbon bonds in organic matter this can release energy for them. These smaller molecules and nutrient elements
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Vapor Pressure and Enthalpy of Vaporization of Water 1/9/12 Emily Toy Lab Partner: Zack Ronnei Instructor: Ms. Olsen‚ AP Chemistry Purpose: The purpose of this lab is to find the vapor pressure of water at temperatures between 50oC and 80oC. Procedure: 1. Take a10 mL graduated cylinder and fill it with 7 mL of water. 2. Next fill a 1000 mL beaker ¾ full with water. 3. Cover the graduated cylinder by putting your finger on top and place the cylinder in the 1000 mL beaker. Make
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2H2O(l) + O2(g). I hypothesize that the speed of the reaction is proportional to the rate of decomposition. Independent Variable The mass of MnO2 used Dependent Variable The rate of decomposition through the amount of mass lost Controlled Variables Environment of the experiment Stay in the same place to carry out the experiment and finish the experiment as fast as possible in case of a sudden change in some areas of the environment Volume of H2O2 used Measure the volume using a measuring cylinder
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Calculating the Enthalpy Change of Reaction for the Displacement Reaction between Zinc and Aqueous Copper Sulphate Data Collection and Processing Observations: * Drops of water left on the inside of the measuring cylinder * Hole in the lid‚ possible escape route for gas or splash-back * The polystyrene cup felt warm during the reaction By extrapolating the graph we can estimate what the rise in temperature would have been if the reaction had taken place instantaneously. I can
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Chemistry Write-Up The Thermal Decomposition of Sodium Hydrogen Carbonate Aim: When Sodium Hydrogen Carbonate (NaHCO3) is heated‚ Carbon dioxide and water are given off to leave a white powder. The aim is to find the equations for this reaction. Hypothesis: The experiment will prove which of the equations below is true. It will tell us whether Sodium Carbonate is produced or Sodium Oxide. 2NaHCO3 Na2CO3 + CO2 + H2O 2NaHCO3 Na2O + 2CO2 + H2O Variables: Independent: Original
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Determination of Reaction Enthalpy Shannon Wedepohl 9/17/13 Abstract: During this experiment‚ an ice calorimeter was used to measure the change in volume in milliliters of magnesium metal and 1.00 M of sulfuric acid. We found the experimental molar enthalpy of the reaction to be ∆H = -370 ± 1 kJ/mol at 0˚C. This compares with an expected value of -466.9 kJ/mol at 25 ˚C‚ a 20.75% difference. Introduction: Many chemical reactions truly only encompass changes by exchanging heat energy
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Chemistry SL Internal Assessment: Enthalpy Change Design Lab Experiment: Reaction of distilled water and solid sodium hydroxide RESEARCH QUESTION How does the heat released during the reaction between distilled water and Group 1 elements (lithium‚ sodium and potassium) vary as one goes down the group? OBJECTIVE The objective of the experiment is to measure the heat change during the reactions with minimal heat loss to the surroundings. MATERIALS The materials to be used in this experiment
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Time Series Analysis: The Multiplicative Decomposition Method Table of Contents Page Abstract………………………………………………………………………………………………………………………………………….3 Introduction………………………………………………………………………………………………………………………...…4-5 Methodology: Multiplicative Decomposition……………………………………………….…5-7 Advantages/Disadvantages of Multiplicative Method………………………………7-8 Conclusion…………………………………………………………………………………………………………………………………..8 Abstract One of the most essential pieces
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Thermochemistry: An Ice Calorimeter Determination of Reaction Enthalpy Curtis M. Franklin Thursday‚ February 14‚ 2013 ABSTRACT An ice calorimetric measurement was used to determine that a reaction involving solid magnesium metal and 1.00M sulfuric acid produces an experimental a value of ∆H = -226 ± 28 kJ/mol at 0°C. This is about 48.4% lower than the expected value reported at 25°C. Introduction Many chemical reactions exhibit themselves by exchanging heat energy‚ either be absorbing
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