Comparision Of Microscale Masses Of Hydrogen And Oxygen

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

This device was able to extinguish small, controlled fires created with an alcohol accelerant, proving that the concept is viable

Write a balanced equation for the reaction of hydrogen and oxygen. You will first need to determine the product for the reaction. (If you have trouble with determining the product, use Google.)

Consumer Products Safety Commission (2001) Fireworks Business Guidance Retrieved on August 24, 2014 from https://www.cpsc.gov/en/Business--Manufacturing/Business-Education/Business-Guidance/Fireworks/

This lab experimented with temperature and gas according to Charles’ Law, which states that gas will expand when heated. The results indicated that Charles’ Law is indeed applicable to this lab. The data concluded that the volume did

In this lab, the molar mass of a volatile liquid is determined based on its physical properties in the vapor state. In order to calculate the molar mass, the mass, temperature, pressure, and volume is measured independently and then converted to the correct units. Sample C was obtained at the beginning of the experiment, which was later informed to be ethanol. Based on the calculations made, the molar mass of the volatile liquid was 95.9 g/mol. However, compared to the known value of 46.1 g of ethanol, the value measured had a 108% error. Unfortunately, this was a very big percent error and may have been caused by incorrectly measuring the volume of the gas. Using the ideal gas law, the molar mass of a volatile compound was calculated in order

A chemical change can be caused by combining two compounds, such as baking soda (NaHCO3) and vinegar (CH3COOH). The change that is taking place is because of the chemical property of reactivity. When these two compounds react CO2 is produced. In this experiment we wanted to see how much baking soda, added to 10mL of vinegar, would cause a film canister rocket to shoot the farthest. I predicted that 10mL of baking soda would shoot the farthest because it would be equal to the amount of vinegar in the canister. The independent variable in this experiment was the amount of baking soda and the dependent variable was how far the lid would shoot.

The burn rate of the mixture was recorded with a video camera and the results recorded and timed. The resulting footage was reviewed and the duration of the combustion noted on a tenth of a second basis. 4 grams of Alliant Green Dot double-base smokeless flake powder with no KClO4 added was also recorded twice in the same manner, to give a baseline burn time and averaged.

The most reactive substance in this lab was the crushed liver core, it produced the most amount of heat, bubbles, and the biggest flame during the glowing splint test. The manganese dioxide and the liver core were also very reactive and they both produced a flame during the glowing splint test. Next, the potato core produced a slight reaction, but it was not as extreme as the other substances. Finally, just the hydrogen peroxide and the boiled liver core had no reaction and did not produce a flame during the glowing splint test.

In a Chinese ritual, tubes made of bamboo filled with gunpowder were thrown into a fire for explosions. After this, gunpowder and tubes have been used for celebrations. As rockets became more advanced, these “fireworks” became more advanced, with more shapes and sizes.

It was desired to compare a theoretical value of enthalpy of combustion to a literature value. To do this, the theoretical value was calculated using a literature value for the heat of sublimation of naphthalene, the heat of vaporization of water and average bond energies, given in Table 1 of the lab packet.1 Equations (1) and (5) were used to calculate the theoretical enthalpy of combustion of gaseous naphthalene, where n was the number of moles, m was the number of bonds, and ΔH was the average bond energy:

The purpose of this experiment was to test and observe the physical and chemical properties of gases, and to use these properties to identify these gases when they are encountered.

Fireworks release an immense amount of chemicals, and have a great amount reactions happen. The reducing agents, sulfur and carbon, combine with the oxygen from the oxidizers to produce the energy of the explosion. Nitrates are usually not used in star explosions, because reactions of nitrates do not produce a temperature high enough to energize many of the more colorful metal salts.In the 1830’s Italian fireworks makers found a group of more explosive oxidizers, which produced temperatures of 1700 to 2000 celcius and made possible the creation of much more intense colors. Unlike nitrate-containing compounds that produce a relatively slow burning rate, the oxidation by chlorates produces a much faster detonation an explosion. The oxygen released

For instance, pentan-1-ol, the alcohol utilised to synthesis 1-pentyl ethanoate, is relatively flammable due to the hydroxyl functional group attached to the molecule. Therefore, in order to prevent severe burns, a laboratory coat and safety glasses were worn. The experiment was additionally performed whilst standing up, so that if the aliquot of pentan-1-ol ignited,

To describe the concept of equal loudness regardless of frequency, the unit phon was developed. Each curve of the equal loudness contours defines a single phon level. For example, the curve that is 40 dB SPL at 1 kHz is defined as 40 phons; 40 phons at 10 kHz is therefore approximately 50 dB SPL and at 100 Hz slightly more than 60 dB SPL. Phons and decibels SPL are the same for a 1 kHz tone — an increase of 10 phons is equal to an increase of 10 dB at 1 kHz, but it may be more or less at other frequencies.