Ethanol Lab Report

The mole is a convenient unit for analyzing chemical reactions. Avogadro’s number is equal to the mole. The mass of a mole of any compound or element is the mass in grams that corresponds to the molecular formula, also known as the atomic mass. In this experiment, you will observe the reaction of iron nails with a solution of copper (II) chloride and determine the number of moles involved in the reaction. You will determine the number of moles of copper produced in the reaction of iron and copper (II) chloride, determine the number of moles of iron used up in the reaction of iron and copper (II) chloride, determine the ratio of moles of iron to moles of copper, and determine the number of atoms and formula units involved in

To prepare and purify an ester: 1-pentyl ethanoate, using pent-1-ol and ethanoic acid. An annotated reaction showing this reaction is shown below:

Introduction: long ago the government banned the ability to make alcohol. This has caused a huge uproar which then people started to boot legging, as more and more people started to drink in the safety of their own homes. After the government saw how people were protesting this new law, they decided that they should left the ban. Since then people were able to drink in public, which in return has created another issue, now that they are drunk at a bar, how do they get home. Rather than taking the safe option and utilize some of the state and local programs and call a tow truck, the Driver chooses to just drive how drunk. They think that it’s ok, since they do not have their full mind.

The graph produced from the Gas Chromatography showed that a reaction occurred because there are peaks on the graph. Each peak represents a major product formed. Since there are two peaks on the graph 2 major products formed. The theoretical yield of the alkene mixture was 3.914 g; however, the actual yield of the mixture was 0.73 g. The percent yield for the reaction was 18.65%. Considering the percent yield, the reaction was not efficient. The difference in the theoretical yield and the percent yield is most likely due to the reaction incomplete reaction. Instead of distilling the reaction to completion, it was stopped after 3 mL of product was obtained. To improve the percent yield the reaction could be taken to closer to completion by continuing distillation past 3 mL of product formed. The low percent yield could also be a result of the extraction. When removing the liquid from the crystals product could have remained behind.

In this experiment, the pKa, dissociation constant, of 2-naphthol was determined by measuring the UV-visible absorption spectra of solution of the acid at different pH values.

This experiment consisted of finding the best ratio of yeast and glucose and of mitochondrial and succinate mixtures to provide the fastest reaction. In both scenarios, the ratio that had equal parts had the fastest reactions. There was very little error in this experiment and any that occurred would have been overshadowed by the vast amount of data collected. Introduction In this experiment, testing different variations of glucose to yeast was done to understand alcoholic fermentation, as well as different variations of succinate and mitochondrial suspension were mixed together to understand cellular respiration.

Fermentation is the anaerobic process by which glucose, or other sugars are catabolized by microorganisms without an electron transport chain, like yeast (Campbell, 2004). In experiment one the yeast and glucose acted as reactants, with the yeast breaking down the glucose, producing the products CO2 and ethanol. The overall reaction for the alcoholic fermentation that took place can be represented as 2 pyruvate + 2NADH-> 2NAD+ +2CO2 + 2 ethanol (Campbell, 2004). This biological process allows cells to operate under conditions where oxygen is not present. Experiment 1 explored the question of how the amount of sugar impacts the rate of fermentation, while Experiment 2 tested the effect the type of sugar available to the yeast has on the rate of fermentation. If more sugar is available to the yeast, the faster the reaction should occur. If sucrose is used instead of glucose, the reaction will produce less CO2 since the yeast cannot breakdown sucrose as efficiently as glucose.

The main purpose of this lab is to determine whether or not the number of carbon molecules relate to the amount of energy emitted measured through the temperature change over the course of 2 minutes. The main three tested fuels are fuels methanol (CH3OH), ethanol (C2H5OH), propanol (C3H7OH). Based on those formulas, Propanol alcohol has 3 carbons, Ethanol alcohol has 2 carbons and methanol has 1 carbon. Based on the hypothesis mentioned above “If the number of Carbon molecules in the fuel increases, the amount of energy over 2 minutes is going to increase”. Based on the data shown above, propanol fuel had the most temperature change meaning that it burned with the most energy. Following that is ethanol fuel having the second greatest temperature

For lab twelve, the molar mass for Isopropyl alcohol is 73.121g/mol. The molar mass for unknown sample is 107.01g/mol. The molar mass for Isopropyl alcohol and unknown sample would be different from true molecular weight because the liquid of Isopropyl alcohol is not completely vaporized in boiling water. There is small amount of liquid left in the Florence flask that affect the result of molar mass for Isopropyl alcohol to be different than the true molecular weight of Isopropyl alcohol. Also, some vapors could have escaped through the pinhole. Instead of making tiny pinhole in the middle of foil, I could have accidently make a huge pinhole that causes the vapors to escape easily and change the result of molar mass. Lastly, I only did one

The purpose of this investigation is to burn selected alcohols of different molecular structure in a controlled environment to compare the magnitude and rates of energy release. Fuels are any kind of substance that, when burnt, produces chemical or nuclear energy that can be used for work. More accurately, fuels may be defined as a naturally occurring or artificially prepared combustible carbonaceous material (Palanna, 2009). One of the most common fuels that is still used today is charcoal. Charcoal is the remains of burnt wood which was discovered to be a good fuel source and was used to melt metals.

The dye extracts obtained in the preceding subsection will be purified by solvent extraction. In this method, equal volumes of ethyl acetate will be added to the concentrated dye extracts. The mixture will then be shaken for a few minutes and put in a separating funnel. A settled solution will have two layers in which the lower layer is the layer of interest. The layer contains mainly anthocyanins.

In the experiment, our purpose is to determine the ethyl ester in an unknown whiskey. We will be using two methods; the first method is called solid phase extraction(SPE) which will be used to separate ethyl ester from whiskey. SPE is based on the selectivity of stationary phase, it will select our desired ethyl ester to stay in the syringe column, and let other molecules go through the column. The second method is GC-MS method, which will help us to identify each ethyl ester. Gas chromatography is based on the interaction between stationary phase and mobile phase, and mobile phase in this case will be ethyl esters. Different ethyl ester has different interactive ability with stationary phase. The bigger the molecule, the longer it will interact

Trial 3 of Ethanol had an error occur, during the experiment the flask fell over causing distribution and causing there to be less fuel burned. This trail was also the only outlier that was detected via using box and whisker plots which are found in the appendices whisker plot 1, 2, 3. Trail 4 in 2-pentanol also had its flask knocked over by the wind, this caused the same effect but not on a large scale to cause it to be an outlier. Another error that was detected in the 2-pentanol trails 8 and 9, this trails had weights that were less than the sprit lamp, this could have occurred due to equipment error (scales) or the reading of the measurement. Another factor that impacted the results is that the spirit lamp flame was not put off as soon

In this investigation I will be burning alcohol 's to heat up a can of water. I will be burning four alcohol 's, methanol, ethanol, propanol and butanol. The aim is to find out how much energy is produced when burning these alcohols. Alcohol 's react with oxygen in the air to form water and carbon dioxide.

During alcohol fermentation, we were assigned a particular yeast strain/beer. Once have figured out which yeast strain/beer your TA assigned you, you needed to pipette 5-10mL in each test tube. We did three treatments with a control for each, which is a total of 6 test tubes. While you filled up your test tubes with beer, you could have had your beaker of water on the burner, waiting for it to reach 99 degrees Celsius. While I was waiting for the water to get to boiling point I placed a test tube rack into a tub to where I was able to create a hot bath. Carefully we ensured two rubber stoppers to one test tube that was in the hot bath and another on the control test tube. Once we have placed the rubber stoppers on the test tubes, open Logger Pro 3.9 to record the temperature at 0,5,15,and 30 minutes. After recording the pressure on our table, I used two different beer test tubes to test for pH. For pH I just spiked the sample with 2mL of acidic solution and then placed both tubs in the warm bath that has now cooled slightly. Then recorded the pH onto the table. But for aeration experiment I want to aerate your beer for 10 min before running. Start the aeration while working on the pH experiment. We used the warm bath to facilitate fermentation again.