Bunsen burner Essays

Students first prepped for the lab by cleaning out the crucible. Three boiling chips were added in the crucible once it was wiped out with a paper towel. The crucible was then placed on a clay triangle two finger widths above the Fischer burner. After 10 minutes of the crucible being directly under the flame, the it was clean and students allowed time for it to cool down. Next, the students from then on used tongs to transport the crucible from weighing it and back to the clay triangle. Now, they

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. To prevent damage to the skin, follow these instructions carefully; tie long hair back, remove any loose clothing or articles that may come in contact with the fire, do not lean over fire, do not leave fire unattended, tidy area around the bunsen burner incase the burner is to tip and begin a fire. After safety precautions have been taken note

To purify metal you have to melt the ore in a crucible, or a container that can resist great heat. A crucible, such as a steel container, clay, and some ceramics can withstand great heat. Crucifixion, the SAT’s and Mr.Maloney's class are all examples of a crucible. Where everyone who enters or gets chosen is severely tested. The Romans placed gladiators in a crucible, a container called a coliseum to fight to the death. I was very contentious with my parents as they wouldn’t let me go to a friends

Wilhelm Bunsen was an influential german chemist that lived during the 1800s. He is known for his significant advances in chemistry in other fields, such contributions towards spectrum analysis , the discovery of Cesium and Rubidium, and his improvement of gas burners in the form of the bunsen burner. Bunsen made significant contributions towards the field of chemistry that remain important to this day. Bunsen was greatly admired in his field for his devotion to chemistry. Robert Bunsen was born

varying professions. Particularly, the engineering of a Bunsen burner is an example of both complete and incomplete combustion at work. Commonly used in school labs to heat chemicals, the Bunsen burner uses natural gas as its fuel, which is almost pure CH4 [methane] (BBC 2011). Since methane is a hydrocarbon, the Bunsen burner is able to manipulate its air hole to achieve both complete and incomplete combustion. When the air hole of the Bunsen burner is open, air is allowed into the chimney. The air then

acid being added to the copper oxide, the copper oxide was no longer visible and the liquid in the beaker turned blue. When the supernatant liquid was removed, the copper was rinsed multiple times and was a red colour. Drying the copper over the Bunsen burner caused it to change colour. I was left with a reddish-brown colour with bits of black and green within. Calculations: n(Cu)=(mass (CuO))/(number of mol (Cu+O))atomic mass (Cu) n(Cu)= 2.00/(63.5+16.00)63.5=1.60 1.76/(2.00/((63.5+16.00)))=69.96 experimental

Aim: to separate seawater using distillation and confirm the identity of the of the major ionic compound present in seawater Materials List 1: Two retort stands and clamps, tile, Bunsen Burner, gauze mat, pear-shaped flask, distillation kit, beaker, two tubes, matches Materials List 2: Tripod, gauze mat, tile, Bunsen Burner, evaporating

flame of a Bunsen Burner. The process of the experiment required extreme precaution, since Bunsen Burners were a key material. Students were given six elements to place within the flame of the Bunsen Burner. Lithium, calcium, potassium, copper, strontium, and sodium were all of the elements used during the process of the experiment. Before the experiment students were required to write a hypothesis. One could hypothesis that the metal elements will change color when put to the flame of a Bunsen Burner

decomposition of this compound by heating this compound under a Bunsen burner. There are four possible equations that will theoretically be used. These equations are as follows: NaHCO3 (s) → NaOH (s) + CO2 (g) 2NaHCO3 (s) → Na2CO3 (s) + CO2 (g) + H2O (g) 2NaHCO3 → Na2O (s) + 2CO2 (s) + H2O (s) NaHCO3 → NaH (s) + CO (g) + O2 (g) This lab will determine the correct

important to know how much sodium bicarbonate could be used if I were to construct my own recipe, to receive a wishful result. Research Question How does the amount, in grams, of NaHO3(s) affect the volume of CO2(g) produced when heated with a Bunsen burner over a time span of 120 seconds, that is, what is the reaction rate of the decomposition for sodium hydrogen carbonate? Background information Firstly, the chemical NaHCO3 has many different names, the IUPAC name is

Year 9 MYP Science Metals Experiment Task Method: 1. Record the number or letter on the container of the unknown metal 2. Use the flame test to find out the metal that is present 3. Note the flame colour 4. If there is no change of colour from the flame, make the substance into a solution by adding deionized water to the unknown metal to make a solution 5. Note the solution colour 6. If the solution is colourless perform the hydroxide test 7. Record your results 8. Now use carbonate test to find

place the crucible with baking soda, on the ring stand, between the clay triangle 6. Set up the bunsen burner right under the crucible held between the clay triangle 7. Then turn on the gas for the bunsen burner 8. Use the striker to light up the bunsen burner and make sure the fire is slightly touching the crucible 9.. Let it sit for 30 minutes 10. Come back and close the bunsen burner 10. Pick up the crucible with tongs, and place it on the balance 11. Weigh the crucible with the decomposed

independent variable was the metal. Thus, the controls were the chlorine (Cl), bunsen burner, deionized water, and cotton swabs used to dip into samples of the metals. Because the bunsen burner was used, goggles were worn and loose clothing or hair was tied back prior to beginning the lab. The first step was to obtain deionized water and 7 q-tips for the 7 metals being examined (Ca, Ba, Cu, Sr, K, Li, Na, and Mg). Then, the bunsen burner was lit to a hot blue flame. Next, a cotton swab was dipped into water

has about 36.0%, and CuCl2 ⋅5H20 (21.17%). Materials: Ring stand, ring clamp, evaporating dish, Bunsen burner, clay triangle, crucible tongs, electronic balance, sample of hydrated salt. Methods: Weight a clean, dry, porcelain evaporating dish on the electric balance and record this mass on an appropriate data table. If the crucible needs to be washed before use, then heat the crucible in the Bunsen burner flame for a few minutes and remove any residual water. Then allow it to cool before continuing

decompose into when heated? Materials: Sodium bicarbonate Bunsen burner Crucible and lid Tongs scale Ceramic fiber pad Striker Stop watch Pipe stem triangle Ring stand Ring clamp Procedure: First The crucible was weighed and recorded for mass. Then you add 2.32 grams of sodium bicarbonate that was measured using a balance and placed in the crucible. The lid was placed on top of the crucible. The crucible was placed above the burner then The burner was ignited, and the flame was adjusted to obtain a blue

Hydrates,” the purpose was to compare the properties of several well observable hydrates and to determine if dehydration is a reversible or irreversible change. The lab consisted of attaining a pea-size sample of each compound, burning it over a bunsen burner, and comparing the starting mass and the mass lost after the combustion. These results are important to be able to identify a variety of different chemicals that contain water molecules as part of their crystalline structure. Some can be removed

First, you place the bunsen burner on the ring stand and tightly place the metal ring and place the clay triangle on it. Before placing the crucible on the ring you must put baking soda in the crucible, and place it on the ring stand. Then with safety precautions light the bunsen burner with the matches provided. In our first experiment we first started with 1.04 grams of NaHCO3 and ended with .60 g Na2CO3

The objective of the experiment was to try to figure out what the mystery powder was. I used a bunsen burner, four different types of liquids. We were given eight powders and one of these powders were our mystery powder. And each powder reacted different to the fire and the liquid. We had to go back into our notes and see what matched to what. Materials I used. Were a petri dish, scapula, liquids, burner, C-clamp, tongs, gas to start the flame, eight different types of powders, and the most importa

gas to excite electrons to a higher energy . the light emitted as the electrons return to lower energy levels will be passed through a diffraction grating and the resulting line spectrum will be observed . in part B I will use the heat from a Bunsen burner flame to excite electrons in solutions of the chloride salts of several metals. The light emitted as the electrons return to lower energy level will not be separated into its compounds. Instead resulting distinctive color of the flame will

ceases, turn off the Bunsen burner and let the crucible cool completely before handling it. Weigh the crucible and record the weight Using a pipette, add a small volume of water to the solids in the crucible Stir the mixture with a glass rod until the mixture forms a paste Return the crucible to the Bunsen burner and heat it for several minutes until all the water has evaporated and the solids have turned light grey → indicating conversion to magnesium oxide. Turn off the Bunsen burner and let the crucible