A hot plate was placed under the ring stand. 50 mL of 3.0 M NaOH in a 250 mL beaker and a stir bar was placed in the beaker. The beaker with NaOH was placed on the hot plate and 3.75 grams of NaAlO2*5H2O was placed in the beaker. The temperature probe was placed in the beaker with the solution, not touching the bottom of the beaker. The solution was heated and stirred till the solution dissolved.
Our objective was to pick the best chemical to be used in a hand warm. This chemical had to be cheap, relatively safe, and must raise the temperature by 20oC and no more. We add 6 different chemicals to water we record the inshell temperature and then add one a the 6 chemicals to the water and record the temperature change of the water. We also add cold water hot water together to find how much heat would escape the calorimeter. We found that the calorimeter absorbed 71.1J/oC. Then this information to calculate the energy that was released by all of the chemical reaction.
It can be hypothesized that the water in the product affected the melting point
During this lab we found the composition of an unknown substance using its melting/freezing point. To do so, we first heated up the substance until it melted, by using a hot water bath. Next, we let it cool at a constant rate while measuring its temperature data using an online program. From this data, we were then able to obtain a melting/freezing point for that data, which was found to be 61.0°C. Once we had that information, we compared it to accepted values of various alcohols and acids.
Utilize a test tube brace to put the test tube containing the obscure strong in the bubbling water shower. Warmth until the greater part of the strong melts. Pour 140-160 mL of faucet water into a 250-mL graduated barrel. Record the volume to the closest 1 mL. Place a buret clasp on a help stand. Gather a calorimeter.
I will put the thermometer into the beaker and stir the water, leave the thermometer till the temperature stays constant.-this will give the normal water temperature. 13. I will take the water out the beaker and wipe it dry. 14. I will activate the heat packs wait for a minute put thermometer onto the copper to see the temperature 15.
The open end of the plastic tubing was twisted firmly into place to the gas pressure sensor. The two-way valve on the rubber stopper was in the OPEN position, and the rubber-stopper assembly was inserted into a 125-mL Erlenmeyer flask. The two-way valve on the rubber stopper was closed. Once the water was boiling, a ring stand and a metal clamp were used to carefully submerge the flask assembly into the boiling water bath. The metal part of the temperature probe was placed into the boiling water.
The Unknown Identification Lab was an experiment that provided the opportunity to apply all the tests that were learned in the semester of lab, to identify the two bacterias that remain unknown. Gram- staining and two other tests will be used to identify the unknowns. This experiment is crucial to the understanding of each test, and can benefit in the ability to identify the characteristics of specific bacteria. Having a clearer understanding of the bacteria can further the research of bacteria for medicine, such as antibiotics. The understanding can also help the development of research in the environment.
Put the beaker with the water and the metal on the wire gauze of the ring stand that has the bunsen burner under it. Fill the graduated cylinder with enough water to about fill the calorimeter and record the amount of water and the temperature of the water that is in the graduated cylinder. When the water starts to boil in the beaker, use the thermometer to record the temperature of the water. Pour the water from the graduated cylinder into the calorimeter. Use the crucible tongs to take the metal out of the beaker and place the metal into the calorimeter and close the
While heat is added at a constant rate, temperature readings will be made until the substance is in its liquid phase at a temperature well above its melting point. The data collected in Parts I and II will be used to construct a graph, which will consist of two curved lines - a cooling curve and a heating curve. When completed, the graph will show pictorially what happens to a pure substance as its temperature is raised and lowered over a temperature interval that includes its freezing and melting points. The graph will also show how the freezing and melting points of a substance are
Part 2 of the laboratory hypothesizes that different PEG precursor combinations will have an effect on the modulus of the material due to the differences in mesh structure. Unlike part 1, part 2 focuses on variation in mesh structure due to the polymerization of 2, 4, and 8 arm PEGnorb with 2 and 4 arm PEG thiol, rather than the impact of polymerization time. Table II displays the precursor combinations, the resulting hydrogel modulus, and the mesh size of experimental groups 1-2, 4-5, and 7-8. Figure 2 (a) and (b) display the modulus of each group and the mesh size of select groups, respectively. Although trivial, the minimum modulus displayed in Figure 2 (a) is group 1, a combination of 2 arm PEGnorb, or PEG 2k, and PEGdithiol, or 2SH, of
4.2 Antifreeze Fluids with IBPs As studies show in Dow Chemical Company (DCC), the glycerol-water solution becomes slushy when it freezes (107) indicated with our studies shown in Figure 41(a). Specifically, the experiment shows the interaction between 20% glycerol and IBPs. For example, at 274.2 K the right-side peak becomes shorter because it reaches its freezing point of the 20% glycerol at 268.5K (83). Then, when the temperature is lowered to 241.1 K, the inhomogeneity of the system due to the glycerol is observed. Studies from DCC has shown that when lowering the temperature, the slush becomes increasingly viscous (107).
In the beginning of the experiment, both planets would have around the same temperature; however, the thinner atmosphere would eventually be hotter, then subside toward the end of the experiment. Two beakers with differing thicknesses of plastic wrap, with a lamp overhead, represents this scenario. According to a group’s data (their group number to be determined), both beakers with differing atmospheres steadily increase by 1℃ respectively until the fifth minute, where the planet with the thinner atmosphere has a hotter surface temperature. After four more trials, the beaker with the thinner atmosphere would increase until both beakers are around the same temperature again. In another group’s data (their group number also inconclusive), both
I. Introduction This experiment uses calorimetry to measure the specific heat of a metal. Calorimetry is used to observe and measure heat flow between two substances. The heat flow is measured as it travels from a higher temperature to a lower one. Specific heat is an amount of heat required to raise the temperature of one gram of anything one degree Celsius. Specific heat is calculated using several equations using the base equation: q=mc∆T II.
Properties of Substances Express Lab 1)The purpose of this lab was to compare the physical properties of different types of solids and how the properties of solids are determined by their intermolecular forces and their intramolecular bonds. Then we were to classify each type of solid as either ionic, metallic, non-polar molecular, polar molecular, or network. Paraffin wax classified as a non-polar molecular, Silicon dioxide was classifies as a network, Sodium chloride was classified as ionic, Sucrose was classified as polar molecular and Tin was classified as metallic. (2)The intermolecular forces that are present in Paraffin wax are dispersion forces, because it is non-polar and carries a negative charge. Followed by Sucrose that has
