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Lab report on determination of specific heat
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Experiment 5 Calorimetry and Specific Heat Lab Partners:_______________________________ February 16th 2017 By: Amanda Luna 1. Abstract The objective of this experiment was to identify a metal based on its specific heat using calorimetry. The unknown metals specific heat was measured in two different settings, room temperature water and cold water. Using two different temperatures of water would prove that the specific heat remained constant. The heated metal was placed into the two different water temperatures during two separate trials, and then the measurements were recorded. Through the measurements taken and plugged into the equation, two specific heats were found. Taking the two specific heats and averaging them, it was then that …show more content…
Take the cardboard cover and place it on top of the two Styrofoam cups, place a thermometer through the small hole in the cardboard cover. This creates a calorimeter. Take the calorimeter and place it into a small beaker to prevent it from falling over. 10. Measure and record the temperature of the water in the Styrofoam cup. Leave cardboard cover on until the heated metal is ready to be transferred into the calorimeter. 11. After the water, has been boiling for 10 minutes, and the temperature inside the test tube has been stable for 5 minutes, record the temperature and remove the thermometer. 12. Quickly and carefully transfer the heated metal from the test tube to the water in the calorimeter. 13. Immediately put the cardboard cover back onto the calorimeter. Stir gently for 2-3 minutes while monitoring the temperature. Record the temperature after it has remained constant for 1 minute. 14. Repeat steps 1-13, but replacing distilled water with colder distilled water (ice water). Trial 2 15. Repeat using the SAME metal sample, but instead with the colder water. Do not record the temperature of the cold water in the calorimeter until immediately before adding the heated metal. 16. Record theoretical values for the specific heat of your metal sample (Table
First, 100 mL of regular deionized water was measured using a 100 mL graduated cylinder. This water was then poured into the styrofoam cup that will be used to gather the hot water later. The water level was then marked using a pen on the inside of the cup. The water was then dumped out, and the cup was dried. Next, 100 mL of regular deionized water was measured using a 100 mL graduated cylinder, and the fish tank thermometer was placed in the water. Once the temperature was stabilizing in the graduated cylinder, the marked styrofoam cup was filled to the mark with hot water. Quickly, the temperature of the regular water was recorded immediately before it was poured into the styrofoam cup. The regular/hot water was mixed for a couple seconds, and the fish tank thermometer was then submerged into the water. After approximately 30 seconds, the temperature of the mixture leveled out, and was recorded. This was repeated three
Using the calorimeter, we firstly needed to calibrate the machine; to do this we took a tube of distilled water and tested it; we knew that this should measure 0 because distilled water is completely transparent. We could have done this with any known reference sample. Once we had calibrated the machine we could then test the real samples for their transparency, we tested all five of these samples a total of three times each. Between each different concentration of solution sample we had to re calibrate the machine using the distilled water again, so in total we did 20 colourimetry tests. We gained three results for each concentration of sample and then calculated an average from these three results; these are shown in the table below.
The purpose of this lab was to calculate the specific heat of a metal cylinder
The procedure of the lab on day one was to get a ring stand and clamp, then put the substance in the test tube. Then put the test tube in the clamp and then get a Bunsen burner. After that put the Bunsen burner underneath the test tube to heat it. The procedure of the lab for day two was almost exactly the same, except the substances that were used were different. The
The temperatures will be set up by using ice to cool tap water down to lower temperatures and boiling water to heat it up. The temperature will be measured to within 0.1°C on a mercury thermometer to ensure accuracy. The temperatures will range from 10°C to approximately 40 °C and it will be done at 5° C intervals.
A thermometer * A clamp * A Bunsen burner * A stop clock Method = =
Distance between the wick and the base of the copper calorimeter: this distance will be 5cm measured using a ruler and adjusted if necessary. The fuel has been weighed correctly: The fuel will be weighed twice, to ensure accuracy. Make sure there is the right amount of water in the copper calorimeter: to make sure the correct amount of water is in the copper I will use a measuring cylinder, I will accurately fill it to 100cm. I will place the cylinder on a flat surface just to check that the measurement is correct. Make sure fresh water has been placed in the container, so that it isn’t still warm and that the copper calorimeter is also cooled down: by making sure that the water has been tipped away straight after the experiment, should hopefully be enough to make sure it will be replaced, also as we have to note the temperature of the water before we start, it should be noticeable.
Tf-Ti). Next, subtract the initial temperature, 25 degrees from the final temperature, 29 degrees putting the change in temperature at 4 °C. To calculate the heat absorbed by the water in calorimeter, use the formula (q = mCΔT). Plug in 50 mL for (m), 4.184 J for (C) and 4 °C for the initial temperature (ΔT), then multiply.
Experimental Summary: First, my partner and I put the marshmallow and cheese puff on T-pins and used the Electronic Balance to measure the mass of each of them. Next, we put 100 mL of water in the 100 mL Graduated Cylinder and poured it into the 12 oz. soda can. We measured the temperature of the water with the thermometer. After
Start with the hot water and first measure the temperature. Record it. 8. Then pour 40 ml into the beaker. You can measure how much water was used by looking at the meniscus.
In this lab, I determined the amount of heat exchanged in four different chemical reactions only using two different compounds and water. The two compounds used were Magnesium Hydroxide and Citric Acid. Both compounds were in there solid states in powder form. Magnesium Hydroxide was mixed with water and the change in heat was measured using a thermometer. The next reaction combined citric acid and magnesium hydroxide in water. The change in heat was measured as well. For the third reaction citric acid was placed in water to measure the change in heat. In the last reaction, citric acid was combined with water. The heat exchanged was again measured. It is obvious we were studying the calorimetry of each reaction. We used a calorimeter
- Temperature was measured after and exact time i.e. 1 minute, 2 minutes, 3 minutes.
By exposing the chocolate and the cookies before the light and heat of the 60-watt light bulb, the students will be able to progressively observe the process of the material melting and make records at every stage of the experiment. Using the 15 seconds step, the students can identify the melt temperature and time of the chocolate under the lab conditions as well as make and analyze their records in the final part of the experiment. The experiment is expected to establish, which of the chocolates and cookies melt faster, and make conclusions about the influence of the consumables ingredients on their physical properties. This corresponds with the TEK 112.11 (5B) procedure, which allows students to “observe, record, and discuss how materials can be changed by heating or
9. When all magnesium has reacted, remove the lid and heat strongly for 5 minutes
4. Put milk samples into the beaker for about five and a half minutes and take samples out after time is up. 5. With the warm samples, open the pouch containing the gel cassette and remove the cassette.