AIM/ OBJECTIVE In this experiment, bomb calorimetry will be used to determine the heat of combustion (heat that the fuel gives off over a certain amount of time when it’s ignited). Determine the Calorific Value of the fuel used and show how the practically determined value compares to the theoretical calculations and industry standards 2. THEORY A bomb calorimeter is a sealed container capable of holding several atmospheres of gas pressure. It measures the enthalpy of reaction by carrying out the combustion reaction under constant volume conditions. This exothermic reaction increases the temperature inside the bomb, which then transfers the energy to the external water jacket raising the external temperature.
Chlorine - Chlorine is an important component of many oxidizers in fireworks. Several of the metal salts that produce colors contain chlorine. Copper - Copper compounds produce blue colors in fireworks. Iron - Iron is used to produce sparks. The heat of the metal determines the color of the sparks.
Materials: 250mL Beaker Test Tube Calorimeter Burner, Ring Stand, and Wire Gauze Thermometer Balance Procedure: 1. Prepare an appropriate data table. 2. Fill the 250mL beaker about half full. Place it on the stand and begin heating it to the boiling point (100 degrees Celsius).
However, in order to accommodate larger samples, the inner width of the reactor was made to be 10 cm that is larger than the standard one (7 cm). The test setup was designed to provide a constant concentration of test gas flow into the reactor and over the sample surfaces. The ambient light was used as an illumination source to test the photocatalytic activity of materials toward nitric oxide. The produced gases in the photocatalytic oxidation of the nitric oxide analysed using NOx analyser (THERMO Scientific Model 42i NO-NO2-NOx Analyser). The experiment was conducted in the following manner: The test sample placed in the photoreactor and, the glass window was attached.
Investigation #2 Flame Tests For Metals When CaCl2 is burned the color of the flame is brick red. When CaCl2 is burned the color of the flame is brick red. The color of KCl is present in a color that is lavande. A mixture of violet and blue. The color of KCl is present in a color that is lavande.
2- Feel the gas on the top of the Bunsen burner with your hands, adjust if too high or too low. 3- Light the Bunsen burner up with the striker. 4- Mix the wool of the Q-tip with your Distilled water. 5- Mix the wool of the Q-tip with your Compound. 6- Place only the edge of the Q-tip at the top the Flame.
The safety goggle was worn. Then apparatus was setup as shown in the diagram. The magnesium was first heated with a small blue flame and after a several minutes with a roaring flame. 5. Every few minutes, the lid of the crucible was lifted carefully with a tong to see if the magnesium had started to burn and also to left some air enter the crucible to make the experiment more efficient.
The lab involved determining the thermal conductivity by electrically heating a sample at one end and water cooling it at the other this gives a linear relationship between temperature and distance form the source which may be manipulated to calculate the thermal conductivity of our material. There is more detail in both the theory and the procedure. This lab has made me consider all the applications of thermodynamics in the modern world and has made me aware of how many applications Introduction The aim of the experiment was to determine the heat conductivity of a substances used. From this result we could determine which substance it was and compare the experimental values to the theoretical.. This lab shows how materials react to heat energy inputs and how far this energy spreads along the substance relative to the energy lost, along with allowing us to calculate the thermal conductivity.
Substances are determined by the characteristics of their flame when they burn. Some compounds produces yellow, sooty flame due to their high carbon content. Some burn with flames that are yellow but less sooty. Infrared (IR) spectrometry gives additional information about a compound