Soot Experiment

1. Which reactants used in this experiment are flammable? Discuss the safety precautions that are necessary when working with flammable materials in the lab?

The purpose of the lab was to determine the ratio of air to acetylene results in complete combustion of acetylene gas. The balanced chemical equation for this experiment was C2H2(g) + O2(g) --> CO2(g)+ H2O(l). Complete combustion is the reaction of an element or compound with oxygen to produce the most common oxides and energy. Complete combustion occurs when the fuel and oxygen combine in exact proportions to completely burn the fuel, which leaves a clean test tube. Incomplete combustion is the reaction of an element or compound with oxygen to produce some oxides with less oxygen than the most common oxides. Incomplete combustion occurs when there is not enough oxygen to react

Please refer to Experiment 5 on page 79-84 of Laboratory Manual for Principles of General Chemistry by J.A. Beran. The only deviation that was observed in the experiment was due to a procedural change instructed by the professor to increase the flame were no observable deviations in the experiment.

The experiment first started by the calculation of the net oxygen production under white light, it started by putting the Elodea in a volumeter tube containing 3% sodium bicarbonate solution, which was assembled to the volumeter by covering the tube with the plug/pipet/syringe assembly (a 1-2cm air space between the bicarbonate solution and the top rubber cover of the volumeter tube should be left.) Then, clamp the volumeter onto the clamp stand using the tube clamp and fill 2000ml beaker with cold tap water. The beaker should be placed on the clamp stand between the volumeter tube and the light lamp. A five minutes stabilization

The luminous yellow flame is smoky because no air is entering the burner and hydrocarbon is converted into carbon dioxide

Other cases involve burning hydrogen and oxygen without carbon and reactions that create carbon monoxide Explain the different between complete and incomplete combustion. What observation can you make to distinguish between the two? Incomplete combustion is also a reaction between oxygen and fuel but the products are carbon monoxide,

However, because the deviation between the oxygen and ideal gas behaviors are very small in the experiment environment and thus can be ignored. So, the ideal gas equation PV=nRT can be used to determine the mole of oxygen generated. Equipment & Reagents Equipment: graduated flask, test tube, alcohol burner, pipette, rubber catheter, glass catheter, glass flume, iron support, dispensing spoon, match, balance, weighing paper. Reagents: KClO_3, MnO_2; (Potassium chlorate, Manganese

I could learn how to identity Hydrogen, Oxygen, Carbon Dioxide, and hydrogen and oxygen mixture when they are present through this experiment. Before conducting this experiment, I should know the combustion chemical reaction first to predict right results. The most interesting thing was the experiment for gases of hydrogen and oxygen mixture. Through the reaction between hydrogen and oxygen, H2O is produced. H2O is water as we know. So I just expected that flame would blow out due to the water vapor. But it was wrong. The flame grew bigger with a pop and a flash.

After the flame of the candle was put off the condensation inside the beaker disappeared this could have happened due to environment error. Another possible error could be when the 15 mL of indicator solution Bromothymol Blue was taken from the beaker that contains the substance. The students did not have an increment of five on their beaker, the level ranged from 10-50mL when the students had to pour the substance into their 50 mL beaker they had to use common sense to figure out how much 15mL. When the students measured the substance they had to be precise, so they could get an accurate result. To see if water is part of a products of a combustion reaction practical errors like the wick of the candle was short and the wick was getting thinner, so heat could not reach the bottom of the beaker this

Koster, E., Koster, K., Berninger, F., Aaltonen, H., Zhou, X., & Pumpanen, J. (2017). Carbon dioxide, methane and nitrous oxide fluxes from a fire chronosequence in subarctic boreal forests of canada. Science of the Total Environment, 601, 895-905. doi:10.1016/j.scitotenv.2017.05.246

There were slipstream soot marks on the right engine nacelle, which identifies as burning in flight. The right horizontal stabilizer had soot and tiny droplets of metal, this shows that the engine was burning during flight.

Overall, the pollution level of smoke was lower than one of sulfur dioxide over the period. Also, both of them increased from 1600 to the end of

Potters created black glaze, used in black figure and red figure styles of vase painting, by changing oxygen levels in their kilns to manipulate color. At around 900 C in a oxygenated environment, all of the clay is red, owning to the ferric oxide (Fe2O3) found in Attic clay (Noble 1965, 32). By using dry wood, the fire produces carbon dioxide gas (CO2), which is nonreactive with the clay allowing it to remain oxidized. Switching to green wood, or damp sawdust, the fire produces carbon monoxide (CO) gas, which will attempt to bond to oxygen atoms to become CO2, “… in this case with part of the oxygen in the ferric oxide in the clay, turning it into ferrous oxide (FeO), which is black” (Noble 1965, 32). Due to the water vapor from the wet wood,

For experiment 100 (pipe flow) there were some operational errors that took place during the lab period. There was one accident that involved the safety officer and the cross trainer that was there for the first lab period. Both the cross trainer and the safety officer were near the viscometer as they were both operating it. When the cross trainer finished utilizing the suction bulb, he was instructed by the team leader to begin recoding the density measurements. The cross trainer reached into the water bath picking up a volumetric flask by its cap, this caused the flask to slip from its cap and fall to the table. While this was happening, the safety officer was crouched near the cross trainer with a stopwatch trying to record the liquids efflux time. As the flask was falling the safety officer reached out to catch it and accidently cut his hand when the flask hit the table. Review attached accident report in the appendix for further detail of the accident.

As with carbon monoxide, nature emits greater amounts of these gases than humans do. The leading natural causes include the decomposition of soil, bacterial activity and lightning. Anthropogenic emissions are mostly due to the combustion of fuel. Natural air is composed of 78% nitrogen and 21% oxygen, which dont react at normal temperatures, but can react if the temperature is hot enough (1300-2500 C). In these cases, the quantity of nitrogen oxides released varies depending on the temperature and the ratio of nitrogen to oxygen. The increasing use of nitrogenous fertilizers is among the reasons that emissions of N2O have been on the rise. Damage to plants by N2O has only been observed near nitric acid facilities and no evidence of NO damage has ever been seen outside the laboratory. It was concluded that the level of concentration of these gases is too low to cause significant problems at this time.