b. Calculate the fuel value in kJ/g for each of these compounds. c. FOr each hydrocarbon determine the percentage of hydrogen by mass. d. By comparing your answers for part (b) and (c), propose a relationship between hydrogen content and fuel value in hydrocarbons. a) for a we first need to find a balanced equation for when the hydrocarbons combust to form CO2 and H20.
In this experiment, the amount of energy (heat) involved in a chemical change will be determined. When alcohol burns it produces carbon dioxide and water as products. Energy is also released in the reaction. The alcohols that will be used are, methanol CH3OH, ethanol CH3CH2OH, propanol CH3(CH)2OH, butanol C4H9OH, octanol C8H18O, and paraffin wax C25H52. The heat obtained when a known mass of alcohol or paraffin wax burns will be used to warm a measured volume of water.
CH 341 – Laboratory Techniques in Inorganic Chemistry Experiment 1: Identification of Stereochemical (Geometrical) Isomers of [Mo(CO)4(L)2] by Infra-Red Spectroscopy Abstract Purpose of this experiment is to prepareone isomer of molybdenum carbonyl complex, [Mo(CO)4(pip)2], and both possible isomers of [Mo(CO)4(PPH3)2] using convenient literature method. Examining the CO stretching region of the IR spectra, the isomers will be identified. Introduction Metal carbonyl considers as one of the most important class of organometallic compounds and many studies of their chemistry and their bonding characteristics has been done (2). Metal carbonyls were first considered as laboratory interests, but soon achieved huge industrial applications (6). The technique of infrared spectroscopy, in both the solid and solution phases, has proved to be of very useful in these studies.
Water samples from the Clark Fork have been taken and will be tested using both absorption and emissions spectroscopy in order to check the levels of group IA and IIA metal ions. When electrons in an element are excited energy is released that can be measured as light. Each element releases different levels of energy that are observed as different wavelengths of light. With the proper equations (E=hv and E=hc/⋋), emission spectroscopy can be used to find the wavelength and frequency of light emitted by the excited electrons. This will help determine the types of ions present in the water sample.
4. Using your definition of substance, classify the following as either a pure substance or a mixture a. ocean water b. air c. granite d. wood e. wine f. liquid nitrogen Part of studying chemistry is being able to form pictures in your mind of what matter looks like on an atomic or molecular level – picturing what kinds of atoms or molecules a particular substance is made of. We can classify the substance based on what types of atoms and molecules it’s made of. We use these images as a way of representing substances. Consider the drawings below: These images show methane molecules (CH4) in each of the three states of matter: solid, liquid, and gas.
Experiment and Observation: Please note that this procedure was adapted from the “Anions, Cations, and Ionic Reactions” LabPaq Lab manual (Hands-On Labs Version 42-0304-82-00-01, 2015) Please reference this manual for further information on the lab experiments. The first experiment was to perform a qualitative anion test. This was done by observation of chemical reactions and recording the results in Data Table 1. Using the information from the reactions we were able to identify unknown substances and recorded the results in Data Table 1. Data Table 1: Anion Confirmation Tests Chemical | Anion | Addition of AgNO3 | Addition of HCl | NaBr | Bromide | Cloudy white thin solution | Clear with sedimentation | Na2CO3 | Carbonate | Clear with white sedimentation | Bubbles, sedimentation combined to one formation | NaCl | Chloride | Milky white, white sedimentation | No visible change | Nal | Iodide | Pale green cloudy, sedimentation | Sedimentation dispersed to smaller pieces, solution clears in color | Na2SO4 | Sulfate | No visible changes noted | Milky white | Na2S | Sulfide | Clear with amber sedimentation | No visible Change noted | Unknown #103 | CarbonateNa2CO3 | Cloudy white thin solution | Bubbles, Sedimentation combined to one
Exothermic and endothermic reactions. First law of thermodynamics and enthalpies of reactions. Calculate standard enthalpies of formations (using the equation on page 191). Electromagnetic radiation, photoelectric effect and continuous and line spectra. Energy levels and electron configurations (including representation using orbital diagrams) of several common elements on the periodic table.
Tammy Thanaporn Amornkasemwong 1st September 2011 Science Period 8 Introduction: How much energy can be released from fuels? Combustion is the process of burning fuel in order to produce heat. The intention of this experiment is to find whether different fuels produce different amount of energy. In the process of combustion in this experiment, cheeto, half a cashew nut, wax candle and ethanol are used as fuels combust with lighter, as heat and oxygen. When the fuels combust, oxygen and fuels react, and heat released.
Experiment 9: Chemical Calorimetry 10/11/12 Group Report Purpose The purpose of this lab was to calculate the change in enthalpy from the chemical calorimetry of magnesium and hydrochloric acid utilizing Hess’s Law to find said change. See summary in equation form below. A. Mg(s)+2HCl(aq)→MgCl2(aq)+H2(g); ΔH=measured in Lab B. MGO(s) +2HCl2(aq)→MGCl2(aq)+H2O (g);ΔH=measured in Lab Use above two equations & thermochemical principles to find change in enthalpy : C. 2H2(s) +O2 (g) →H2O (l); ΔH=-571.6KJ Hess’s Law of heat summation to predict the enthalpy change of the reaction: D. 2Mg(s) +O2 (g) →2MgO(s) Procedure Followed lab procedure as outlined in Chemistry 1127 lab manual, experiment #9. Results Table 1: Water Temperatures Calorimeter Trial # | Cold Water Temp °C | Hot Water Temp °C | Plateau Temp °C | C: Calorimeter (J) | 1 | 23.5 | 42.4 | 30.8 | 61.0 | 2 | 24.8 | 55.1 | 36.8 | 54.9 | 3 | 24.9 | 60.6 | 38.7 | 61.4 | Average Heat Capacity: 43°C/J Table 2: Mg Reaction Data Mg Reaction | | Trial 1 | Trial 2 | Trial 3 | Mg mass (g) | 0.1506 | 0.1503 | 0.1506 | Dry Calorimeter mass (g) | 30.84 | 30.80 | 30.82 | 0.10 M HCl mass (g) | 25.45 | 24.79 | 25.15 | Initial HCl Temperature (ºC) | 22.5 | 22.7 | 22.5 | Plateau HCl Temperature (ºC) | 55.6 | 45.4 | 46.4 | Reaction (kJ) | -4.93 | -3.42 | -3.49 | ΔH Mg (kJ/mol) | -740 | -550 | -560 | Average ΔH: -620 kJ/mol MgO Reaction | | Trial 1 | Trial 2 | Trial 3 | Mg mass (g) | 0.2504 | 0.2507 | 0.2516 | Dry Calorimeter mass (g) | 30.95 | 31.12 | 31.06 | HCl mass (g) | 25.09 | 24.63 | 24.61 | Initial HCl Temperature (ºC) | 22.7 | 22.4 | 22.5 | Plateau HCl Temperature (ºC) | 28.9 | 29.8 | 32.7 | Reaction (kJ) | -1.04 | -1.08 | -1.04 | ΔH Mg (kJ/mol) | -178 | -169 | -238 | Average ΔH: -200 kJ/mol Calculations
Its esters are also used as solvents for inks, coatings and paints. Mechanism of Acetic Acid Acetic Acid is produced through a process called Methanol Carbonylation where Methanol and Carbon Monoxide react, resulting in Acetic Acid’s production, as demonstrated in the equation below: CH3OH + CO → CH3COOH Another method of using Methanol Carbonylation to produce Acetic Acid requires an intermediate – iodomethane – and a catalyst – Metal Carbonyl, for carbonylation. The equation used for this process is as follows: CH3OH + HI → CH3I + H2O CH3I + CO → CH3COI CH3COI + H2O → CH3COOH + HI There are other methods used in the production of Acetic Acid, though they are not as popular as Methanol Carbonylation, as listed below: Acetaldehyde Oxidation Ethylene Oxidation Oxidative Fermentation Anaerobic Fermentation References: Wikipedia, the free encyclopaedia en.wikipedia.org/wiki/Acetic_acid Credits: Jimmy Donal Wales Sir Timothy John Berners-Lee Glossary: Polyvinyl Acetate (PVA) – A rubbery synthetic polymer Cellulose Acetate – The acetate ester of cellulose Ester – Chemical compounds consisting of an ether linkage adjacent to a carbonyl Methanol – By-product of the destructive distillation of wood Carbon Monoxide – A colourless, tasteless and odourless gas that is less dense than air Intermediate – A molecular entity that is formed from the reactants