Methanol Alcohol And Ethanol Lab

In this experiment, the results of the tested materials gave off heat and the change in the temperature was positive because when one substance was added to another the temperature increased. A calorimetric constant is required because the calorimeter that was made is different for every lab group.

he experimental variable in this experiment was the changing number of Alka Seltzer tablets that were put into the 250mL beaker of vinegar. Some of the control variables in this experiment were that the same beaker and thermometer were used for each trial, the same type of vinegar and Alka Seltzer were used for each trial, and the same amount of vinegar. The original Hypothesis was that more Alka Seltzer would increase the temperature of the vinegar was not correct. After analyzing the data it can be seen that for the first trial the temperature did not change as it stayed at 24 degrees Celsius before and during the reaction with 1 tablet, also for trial two with two tablets the temperature stayed the same at 23 degrees Celsius and did

I will measure these individual alcohols by mass which will be measured in grams, I'll be making two readings of each alcohol before the experiment and after, which would tell me the mass lost and how much heat is produced. Dependent Variable, the things that I'll be measuring would be the temperature (oC) increase at the start and the final resting point once combustion has been stopped of each different alcohol being lit to heat the water in the copper calorimeter, and the mass before and after the experiment of alcohols. Fixed Variables, the things that I have chosen to keep the same in each individual experiment to keep it a fair test, is to keep the same amount of water being heated, the same copper calorimeter, as it may vary in conductivity, the height of the calorimeter, and the same amount of time for each

In this lab, there are two days. In the first day, there are is part A and part B. Part A is further divided into three experiments. In experiment one, we were to figure out the heat capacity of the calorimeter that we made. The next two experiment’s goal was to calculate the enthalpy of 2 reactions and using hess’s law, figure out the heat of formation of magnesium oxide. In a reaction, there are

The experiment answered the question; How do yeast metabolize different fuels? My hypothesis was that yeast could metabolize some fuels and not others, but all the fuels would be metabolized at a different rate. My prediction was that yeast could metabolize all the fuels we used, but it would metabolize at different rates. Yeast metabolizes different fuels by fermentation without the presence of oxygen; this is the method we used in the lab. The control group produces carbon dioxide because there are still different sugars in the water. These sugars are there because we used normal tap water, which contains many different molecules and ions inside the solution. It is important to have the control group to compare to the other fuels because we can see how much the other fuels have created compared to the normal water from the

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From the data analysed, a clear trend is seen. As the amount of carbon chains (and consequently molar mass) increases, so does the heat of combustion released. The hypothesis was stated as: “because 1-hexanol has more carbon bonds, it will produce the most amount of heat in the shortest period of time. By following the same reasoning, it is suggested that 1-hexanol will be followed by 1-pentanol and 1-butanol, respectively.” The experimental values show there is a linear relationship between the carbon chains and molecular weight, and the heat of combustion

In this experiment, the relative rates of free-radical chain bromination where determined. Five arenes were used for this comparison along with two controls for each set. One set was kept in the dark while the other was put under light. This allowed for better observation of the reactions, as the light set would proceed fast to show which arenes reacted slowest, while the dark set would proceed slowly to show relative differences between the faster reacting arenes. The time it took for the arenes to react was recorded to determine the relative rates of the reactions.

In a 100-mL beaker, 6.0 mL of concentrated sulfuric acid (H2SO4) was cooled to 0 ˚C and then 3.05 g of methyl benzoate (C6H5CO2CH3; density=1.08 g/mL) was added. In two different beakers, 2.0 mL of concentrated sulfuric acid and 2.0 mL of concentrated nitric acid (HNO3) were cooled in an ice bath. Both acids were mixed together and the mixture was allowed to cool in the ice bath. The mixture in the 100-mL beaker was cooled to 0 ˚C. While still remaining in the ice bath, the acid mixture was slowly added into the methyl benzoate solution by the use of a Pasteur pipet. The temperature of the solution was controlled by swirling the solution and stopping the addition of acid mixture when the temperature raised.

Three sources of error that might have led to the systematic error during the lab include: lack of insulation, lack of even heating, and loss of heat to the environment. First, in my experiment I had to set the sample foods aflame in a coffee tin, which would heat the water inside the soda can. There was a large amount of heat that escaped through the top of the soda can, which made the water have a smaller temperature change. Secondly, there was incomplete burning of food in my experiment. The marshmallows did not burn; instead they caramelized on the outside, so not all the energy contained was released. Incomplete burning also occurred with the animal crackers. Lastly, my inefficiency was caused by heat loss to the environment. When trying

The effect of metals supplementation on methanogenesis was studied to confirm whether could increase methane production. Ion metals as trace elements were proven to enhance biogas formation during anaerobic oxidation of organic matter [37]. However, its efficiencies are varied and depend on many factors such as the biogas system, inoculum source, metals used, etc. Three concentrations of metals (i.e., Ni, Co, and Fe) at three different concentrations of each metal were tested using granular sludge as inoculum. The metals concentrations that proven that could enhance methanogenesis would be utilized for later experiments with M. barkeri. Since dechlorination by methanogens is believed via co-metabolism pathways, it was assumed that higher methanogenesis activity would result in higher dechlorination rate.

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.

In conclusion, the marble that made it to the bottom of the tube the fastest in the substance was isopropyl alcohol. The marble in Isopropyl alcohol took 1.16 seconds to get to the bottom of the tube. Isopropyl alcohol was the fastest because, It contains 1 H and the H bonds with 1 O therefore, it has a less viscosity so the substance is less thick so the molecule travels through the liquid fastest. The second fastest tube was ethylene glycol it has 2 H’s that bond with 2 O’s it has more H bonds then isopropyl alcohol so it has a greater viscosity which means it takes a longer time for the marble to travel through the substance because it’s less liquidy and it took 1.59 seconds. The slowest tube was glycerol. Glycerol has 3 H’s that bond with

We will be using 6 different fuels to heat up 100ml of water, and find out the changes of the temperature. We will measure the temperatures of the water before and after the experiment. We will burn heat the water for exactly 2 minutes, and check the changes in temperature. The change in temperature will allow us to work out the energy given off the fuel by using this formula:

The results that were revealed were thought to be accurate and reliable as many factors were controlled to enable the best quality. The results that a constant rise in the combustion occurred as each alcohol’s carbon chain increased with one exception indicates that the reliability of this experiment has to be examined. With such a high percentage error from these results means they cant be definitive. Also only three trials were conducted on the five different alcohols. If the experiment were to be conducted again I would conduct five trials on each alcohol to get a better average.