Rapid Oxidation of Steel Wool Arby D. Dickert Western Governors University Rapid Oxidation of Steel Wool Abstract The rapid oxidation of steel wool involves an exothermic reaction of iron with oxygen. Due to the decrease in volume of the combustion products compared to the original sample, many students would expect the products would weigh less than the original sample. This investigation determines that the product weighs more than the sample and why this occurs. In addition, properties such as color and magnetism provide additional identification. Keywords: combustion, steel wool, iron, magnetite, ferric oxide When a candle burns, the wax disappears. When wood burns, the wood is reduced to ash to about ten percent of its …show more content…
In addition, we can predict the percentage increase and use this information to help define the combustion product. Furthermore, we can use the color as well as magnetic properties of the combustion product as additional evidence. In the Astro-Venture course, NASA developed an excellent presentation and experiments for oxidation and combustion. In the course, NASA (2014 p. 119) explains what happens when iron rusts in the presence of water: 4Fe + 3O2 form 2Fe2O3. Four atoms of iron combine with 3 atoms of oxygen to yield two atoms of ferric (iron) oxide. Ferric oxide is formed when iron is oxidized at low temperatures. The ferric oxide is distinguished by its red color. Combined with other substances it is used as a color in paint. Note that the oxygen has now combined with the iron. This implies that the combustion product contains more elements and should have more mass than the original. Ferric oxide is not attracted to a magnet and is not attracted to …show more content…
The aluminum foil and the steel wool were taken outside onto a concrete driveway and ignited using a match. As the steel burned, I blew on the steel wool to make sure all the steel wool was consumed. I made sure that I did not blow too hard and scatter the combustion products. After making sure that the fire was out and all the fuel was consumed, I brought the aluminum pan now containing the combustion product inside and allowed it to cool to room temperature. Once the aluminum pan and combustion material reached room temperature, I weighed the pan. The results are show in Table 2. We can predict the results we should see using the following equation for the oxidation of iron into magnetite: 3Fe (s) + 2O2 (g) → Fe3O4 (s) Three units of iron with a mass of 56 plus four units of O with a mass of 16. This yields a magnetite combustion product of (3 x 56) + (4 x 16). In other words, 168 units of iron combine with 64 units of oxygen yielding 232 units of magnetite. The oxygen added accounts for a 38% increase in the mass. Instead of the mass of the being reduced, the chemical formula predicts an increase. Similar calculation performed for ferric oxide show a 43% increase in mass. See Table 1 for the predicted percent increase. Thus the percent change in mass may be an indicator of the combustion
While the solution dissolved, 50 mL of distilled water was added to a 150 mL beaker and heated on the hot plate. When the solution started to boil 2.65 grams of Na2SiO3*5H2O was added to the beaker with a stir bar and heated to a gentle boil. When both solutions began to boil, the sodium silicate solution was slowly added to the sodium aluminate. The solution was kept at 900C for 60 minutes and stirred with stir bar. After 60 minutes, the zeolite solution was cooled for 5 minutes and for the magnetized zeolite , 0.78 grams of FeCl3 and 0.39 grams of FeSO4*7H2O was added to the flask and stirred until the iron parts dissolved.
Consequently, it induces second element to be oxidized. 2. In the experiment #3, zinc electrode acts as anode, where the oxidation processes occur, while iron half-cell acts as cathode, where the reduction processes appear. In the experiment #4, iron is visa verse reducing agent that evicts electrons to copper half-cell through the circuit.
Then more roasting occurred when the crucible was placed into a ceramic triangle for the Bunsen burner to continue its burning for an additional 90 minutes. Once the burning was officially over, the crucible was placed onto a ceramic tile to cool off. Next the charcoal and copper material were poured onto a paper towel and were separated from carefully distinguishing them one from the other. Then comparisons were down through analysis of the copper (II) oxide smelted.
(i.e., what was the evidence of reaction?) When the piece of magnesium come in contact with the flame, it ignited and emitted an intense bright white light. The light was so intense that it was painful to look at. Furthermore, after the metal was done burning the piece of magnesium changed color and consistency. Before the reaction it was a dull gray, malleable piece of metal.
Josh Powell person of interest, Mr. Powell got custody of the two children, Josh's father stayed with Mr. Powell, Steven Powell was arrested on charges of voyeurism and child pornography in 2011, 2011 Susan's parents were granted custody of the boys, Josh ordered to undergo psychological testing and polygraph testing, Powell let boys in locked CPS worker out, CPS worker smelled gas. Now that I have all the notes I need I can now proceed to investigate the fire. Based on the four stages of fire I have found that incipient stage just made the duration of the fire spread more than a fraction it speed very quickly due to the product that was used. Emergent smoldering to effect very quickly make thing more combustible.
Wax is a block of chemical compounds mixed together to make the wax. There are two different kinds of wax, Paraffin wax and Beeswax. A wick is usually made of braided cotton, used to burn a candle or an oil lamp. The wick of the candle influences the burning of the candle. Data: The coloured candle burned slower than the white candle.
In the picture below we get a better understanding of how much ash would fall in the surrounding vicinity measured in terms of
Fire is a hazard that continues to claim many lives annually; it remains an untamed emergency and will affect the elderly significantly. Once a fire starts in any place the elderly may have less chance to run away from the fire or call fire emergency to respond to the fire, they are therefore more vulnerable to injury and/or death caused by the fires. People will normally die from being overcome by gasses, smokes or toxic fumes, while others will suffer from burns. Factors such as poor mobility, reduced tolerance to smoke and burns, reduced sense of smell are some that contribute to exposing the elderly to fire fatalities. Additionally most of the elderly will live alone in their homes and hence in case there is a fire they may find it difficult to move out or reach the telephone to notify the fire department.
Chemical compounds that are available to determine are CaCO3, CaCl2, Ca(NO3)2, mgCl2, MgSO4, KCl, HCl, HC2H3O2, KNO3, K2SO4, NaC2H3O2, Na2CO3, NaCl, Na2SO4, HNO3, H2SO4, HNO3, H2SO4, NH4Cl, (NH4)2SO4, K2CO3, 0.1 M AgNO3, 0.2 M BaCl, Mg(s), NaOH, and KOH. To start this experiment, start with the flame test by gathering a Bunsen burner and a Nichrome wire. Connect the Bunsen burner with a rubber tube to a laboratory gas. To prepare solutions for the flame test, weigh out 0.205 gram of Unknown Compound using an analytical balance and mixed it into a 140 mL beaker filled with 20 mL ionized water. Ensure that solid is completely dissolved using a stirring rod.
Copper Cycle Lab Report Ameerah Alajmi Abstract: A specific amount of Copper will undergo several chemical reactions and then recovered as a solid copper. A and percent recovery will be calculated and sources of loss or gain will be determined. The percent recovery for this experiment was 20.46%.
The percent recovery of the copper was calculated using the equation, percent recovery = (the mass of the copper recovered after all the chemical reactions/the initial mass of the copper) x 100. The amount of copper that was recovered was 0.32 grams and the initial mass of the copper was 0.46 grams. Using the equation, (0.32 grams/0.46 grams) x 100 equaled 69.56%. The amount of copper recovered was slightly over two-thirds of the initial amount.
Introduction: This lab report discusses an experiment to study the difference in the burn rate of various colored candles. The objective of this experiment is to analyse the outcome of burning 5 different colored candles including white under the same control variable for 60 minutes. The white candles used in this experiment are pure and no chemicals or dyes are added to it. They are normally made from paraffin wax with a wick in the middle.
℃^(-1)×6.40℃±3.1 %=1337.6 J±4.06 % ∆H=(-1337.6 J±4.06 %) /(0.025 mol ±0.16 %)= -53504 J m〖ol〗^(-1)±4.22 % ∆H=-53504 J m〖ol〗^(-1)±4.22 %÷1000=-54 kJ m〖ol〗^(-1)±4.22 % Conclusion and
This method is called oxygen candles. It burns iron and chlorate mixture powder together at about 600 Celsius to produce Oxygen gas (O2), salt (NaCl) and iron oxide (FeO) (Freudenrich). Other than oxygen, we can also produce salt as well by using this method. Bibliography: Dunbar, B. (n.d.).
The Calorimeter Calorimetry is the science that was first recognized by a Scottish physician and the scientist Joseph Black. It is related with determining the variation in energy of a system by measuring the heat transfer with the surrounding. It is derived from the word calor in Latin, which means the heat and the pressure. Calorimeter is the device used in the calorimetry science to measure the quantity of heat transported from or to an object. Heat is the transfer of thermal energy between two bodies that differs in temperature (Mc Graw Hill Education).