Ethyne Gas Combustion Reaction Lab

In a Beacon School, located in NYC, two-tenth - graders were seriously injured, leaving a boy with critical burns and another student with fewer server burns from her neck, head, and arm. Anna Peole, chemistry teacher was showing a “demonstration of rainbow flames” which will result burning of 4 different kinds of nitrates in separate crucibles in the classroom. However, the unstable amount of methyl alcohol hazes around the chemistry lab and explodes across the lab table surrounding Alonzo Yanes, a sophomore at the Beacon School. Alonzo Yanes was standing a few feet away from the lab table, where the crucibles were.

Weighed 1 gram of NaC2H3O2 and mixed it with ionized water. Boiled 12 mL of 1.0M Acetic Acid added into a beaker containing the sodium carbonate on a hot plate until all the liquid is evaporated

In this state they can then readily react with oxygen in the air, which gives off enough heat in the subsequent exothermic reaction to vaporize yet more fuel, thus sustaining a consistent flame. The high temperature of the flame causes the vaporized fuel molecules to decompose, forming various incomplete combustion products and free radicals, and these products then react with each other and with the oxidizer involved in the reaction. Sufficient energy in the flame will excite the electrons in some of the transient reaction intermediates such as the Methylidyne radical (CH) and Diatomic carbon (C2), which results in the emission of visible light as these substances release their excess energy (see spectrum below for an explanation of which

Record initial temperature of water 4. Fill spirit burner with 50ml of 1st fuel and weigh 5. Place spirit burner under the tripod 6. Light spirit burner and let burn under beaker of water for 30 seconds 7. Once 30 seconds is reached, record final temperature of water and put the lid on the spirit burner to stop flame and remove from apparatus 8.

In this experiment we will be looking at the effects that combustion has on the air around it and the bi-products that it produces in a confined space. I will be asking the question of why fire fighters have to crawl in a burning building and what must be done when someone is stuck in a burning building. The experiment will showcase the following chemical reaction: Fire + Oxygen + Hydrocarbons => Carbon Dioxide

Use a stopwatch to track the time of the combustion of ethanol. While the water within the beaker is being heated, use a stirring rod to stir it. Put the fire out when 4 minutes have elapsed. For safety precautions, let it cool off a bit before using the scale to measure and record, the final mass of the alcohol burner containing the ethanol.

This reaction is an acid base reaction thus results expected to show some carbon dioxide. Method: A 20ml vinegar is poured in the 250ml bottle. A funnel is used to pour 3g of baking powder in the balloon by sticking the funnel in the neck of the balloon to easily allow the baking powder inside without it spilling on the sides. Slowly but surely the balloon is placed on the mouth of the bottle by stretching it gentle so that it does not tear. A 10cm string is used to tie the balloon on mouth of bottle so that air may not intrude and no air formed be lost.

Measure 10 ml of .5 M HCl (measure from meniscus) using a pipette into a clean dry measuring cylinder and pour into a clean 100 ml conical flask. Repeat step 5 and 6 for 1M and 2M HCL and keep all the acids ready away from working bench to avoid spills during experiment. Reset your stopwatch timer and prepare a gas delivery system including water bath as shown in apparatus below.

Also, I expect the combusting to give of a burning smell, similar to an explosive. At the molecular-level when a firework goes off molecules will begin to exchange electrons due to increasing levels of temperature (must be ignited

Cooling process: By cooling down the material through some chemical reactions in which energy absorbing (endothermic) processes triggered by additives and/or the chemical release of water cool the substrate to a temperature below that required for sustaining the combustion process, e.g. magnesium hydroxide [26,13,20]. Coating process: By forming a protective layer or coating that prevents or shields the underlying combustible layer of material with a solid or gaseous protective layer from heat and oxygen necessary for the combustion process, e.g. phosphorous and boron compounds [26,13,20]. Dilution process: By incorporating inert substances (e.g. fillers) and additives that release inert gases, water or Carbon dioxide during decomposition, and dilute the fuel in the solid and gaseous phases so that the lower ignition limit of the gas mixture is not exceeded, e.g. aluminium hydroxide leaving water [26,13,20]. Fire retardation by Chemical action The most significant chemical reactions that interfere with the combustion process take place either in the solid and gaseous phases: Reaction in the gaseous

o Last updated: Sep 23 2009  http://www.scientificamerican.com/article/what-is-an-exothermic-rea/ o Date of use: 15 February 2015 o By: Van Hecke G.R. o Last updated: 27 September 1999  http://chemistry.about.com/od/endothermicexothermic/ss/Exothermic-Reaction-Examples-Exothermic-Demonstrations-To-Try11.htm#step-heading o Date of use: 15 February 2015 o By: Helmenstine A.M. o Last updated: 5 February 2015  http://www.sciencedirect.com/science/article/pii/S036012859000598 o Date of use: 15 February 2015 o By: Zeng K. and Zhang D. o Progress in Energy and Combustion Science, Volume 37, Issue 5< September 2011, Page 631  http://www.ngopulse.org/article/use-gas-safely-home-summer o Date of use: 15 February 2015 o By: Kulati P. o Last updated: 3 December 2014  http://www.propane101.com/carbonmonoxideandpropane.htm

Modernized homes across the planet generally utilize paraffin wax as an alternate source of light in case the power goes out. Understanding the heat of combustion of a lit candle will allow people the knowledge of how effective a candle really is. This lab on the heat of combustion of paraffin wax tests students on their ability to use the previously mentioned ideas and concepts as well as their understanding of calorimetry. The students will calculate the efficiency of a paraffin wax candle and a material of choice by determining the heat of combustion. Fully understanding calorimetry is a very important skill to have whilst analyzing fuels.

After adding three boiling chips, 10 mL of 48% hydrobromic acid was also added to the round bottom flask and swirled for 15 seconds to reactants in the flask. The reactants were clamped to a ring stand and a pre-set reflux apparatus with clear hoses attached to the condenser. The voltage regulator was set to 40 to begin water flow through the condenser and the application of heat, so the solvent can boil. The reaction was set to reflux for 30 minutes.

Explain the sequence of thermal stages involved in combustion from preheating and to flaming and glowing. Identify which of these steps are endothermic and which are exothermic. Burning begins with endothermic reactions that absorb energy and ends with exothermic reactions that release energy. The endothermic reactions are known as preignition, the exothermic reactions as combustion, and the point of transition as ignition.

In this lab certain safety precautions must be followed, these include wearing goggles at all times to protect the eyes from any dangerous chemicals, hot objects, acids, or glass wear should all be handled with care. If any chemical is to become in contact with skin, be sure to wash the affected area with soap and water immediately. Any mixtures should not be disposed until instructed. Before use of any equipment be sure that all equipment has been properly cleaned, otherwise chemicals used prior to this experiment may be remnant. When using the bunsen burner safety precautions must be taken seriously as one could easily be burnt.