Simple and Fractional Distillation of Cyclohexane and Toluene Purpose: The purpose of this experiment was to become familiar with the processes of simple and fractional distillation. In this experiment a mixture of two volatile compounds, cyclohexane and toluene, were separated with the process of distillation. Distillation relies on each compound having distinct and separate boiling points. The pure products were analyzed with gas chromatography to determine the success of the distillation. Introduction: Distillation is the process of heating a liquid until it boils, then condensing and collecting the resulting hot vapors.
Energetics Aim: To measure the energy released from the complete combustion of a known mass of alcohol or paraffin wax, to heat water. Hypothesis: The combustion of alcohols is exothermic. In this experiment the energy is released from burning a known mass of alcohol in order to heat a known amount of water. A comparison of various alcohols and paraffin wax (methanol, ethanol, propanol, butanol, octanol and candle) as fuels can be made by calculating the quantity of energy transferred to the water. In this experiment, the amount of energy (heat) involved in a chemical change will be determined.
Add 1 mL of deionized water to the small test tube containing the precipitate and mix it and centrifuge it for 60 seconds. Then, add the supernatant into the boiling test tube and repeat this step one more time with another 1 mL of deionized water. Acquire a pair of metal test tube holders and heat the boiling test tube to evaporate the water for 15 minutes. Let is cool after and weigh it. Then, calculate a percent yield of zinc iodide and write a balanced chemical equation and determine the limiting
When the fuels combust, oxygen and fuels react, and heat released. The water then absorbed the heat from the combustion. In this experiment the calorimeter of energy is used to measure the temperature of the heat that is released from the cashew. The equation to find the energy produce during
5mL of acidified water will be measured, using a graduated cylinder, and will be transferred to the R tube, and will be immediately vigrously mixed with the reactants. Once the solution turns to an orange or red-brown color, a pipet will be used to quickly remove 30 drops of the solution, then transferred to the C tube, and the mixing will resume until the solution is close to room temperature. The solution will be filtered into the P tube, and the solution that is left in the R tube should be washed three times with 1mL of acidified water each time. The water should then be poured into the P tube, leaving the solid in the R tube. Using a test tube holder, heat the R tube over the Bunsen burner, moving the tube in a circular motion until all the water has evaporated.
By using this method of distillation a mixture is heated to a temperature at which several fractions of the compound is evaporated the distillate is then condensed and collected. Generally the component parts have boiling points that differ by as little as 20-30°C under a pressure of one atmosphere. However, cyclohexene and cyclohexanol have boiling points of 83°C and 161°C, respectively, and fractional distillation was used to separate the starting material from the desired product. The mixture is heated and boiled and the vapors produced are condensed and the distillate is collected and then tested by GC analysis. The Agilent 7890A Gas Chromatography System separates chemicals based on the ease with which they evaporate into a gas, also known as the volatility.
Abstract In this experiment we are explored the simple calorimetric estimate for the enthalpy of combustion of different alcohols. Our aim is to find out which alcohol is most efficient. Method First of all we drew up a table – this was what we used to record our results in. We then measured 100cm3 of water into a measuring cylinder and poured the water into steel we then recorded its temperature. We selected a spirit burner and recorded the name of the fuel into our table; we also included the mass of the whole burner.
The first was done by setting up a Reflux apparatus in order to heat the reaction mixture which contained 2.5mL of isopentyl alcohol, 3.5mL of glacial acetic acid, and 0.5mL of concentrated sulfuric acid(catalyst). The mixture was left to boil for 60 minutes(1hr) with a boiling stone inside the heating vial for mixing. After completion of the heating process, the vial with the product was left to cool to room temperature. The next step was to extract the organic layer of the product. First, the product was transferred from the heating vial to a centrifuge tube
When the gas comes out of the ground, it comes out wet. The first stage of the refining process involves on-site heating of the gas to 212 degrees to evaporate any non-methane hydrocarbons and fluids that are mixed into the gas. (Arthur, 2008) The condensate that is generated from this process is then vented into the atmosphere. The condensate often contains the same chemical additives that are added to the well during the fracking process, as well as volatile organic compounds that are naturally occurring in the ground where the gas is stored (Witter,
CaCO3 + 2HCl -----CaCl2 + CO2 + H2O ( Volume of acid added (L) ) (1.0mol/L) = moles acid added. Moles acid added - moles base added = moles acid that reacted. Moles of acid that reacted / 2 = moles CaCO3 present in sample. Final answer % CaCO3 3. Put exactly 5.0 mL of water in the 10.0 mL graduated cylinder.