Determining Specific Heat of a Metal Sample
1. Obtained the metal sample from Dr. Rogers
2. Placed a 400 mL beaker that is 2/3 full of water on a hot plate in the fume hood and brought the water to a boil. While the water was boiling, weighed and empty weighing boat then took the solid metal sample and weighed it in the weighing boat. Recorded the two weighs and subtracted the values to calculate the mass of the metal.
3. After calculating the mass, poured the metal into a test tube and placed the test tube in the boiling water for approximately 10 minutes.
4. While allowing the water to boil, the mass of an empty calorimeter was measure on the analytical balance along with the mass of that same calorimeter filled with 40 mL of water. Once the mass of the calorimeter with 40 mL of water was weighed, the calorimeter was placed on a ring stand and the temperature of the water within the calorimeter was measured and recorded.
5.
…show more content…
After 10 minutes was up, the test tube that contained the metal sample was removed from the boiling water using a folded paper towel to grasp the beaker. The test tube was then dried with a second paper towel and the metal contents were poured into the calorimeter. The thermometer was taken and placed within the calorimeter and that metal was moved around inside of the calorimeter to change the temperature of the water. The highest water temperature observed was recorded.
Density - Another Physical Property
1. Placed 30 mL of water within a beaker and placed the metal sample within the beaker. After placing the metal sample within with beaker the volume of water in the beaker changed. The volume change was recorded for the volume of the metal sample.
2. The volume of the metal sample was placed into the density formula along with the mass of the metal sample to calculate the density.
Determining the Density of
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
Theory of Water of Displacement: A volume of water was measured. A second volume of water was measured when the metal cylinder was added. The initial volume was subtracted from the second (total) volume to get the volume of the metal cylinder.
It was learned that changing the volume of the same substance will never change the boiling point of the substance. However having two different substances with the same volume will result in two different boiling points. The purpose of this lab was to determine if changing the volume of a substance will change the boiling point. This is useful to know in real life because if someone wanted to boil water to make pasta and did not know how much water to
6. Place the test tube in the beaker. Secure the test tube and thermometer to the retort stand using clamps. Begin heating the water bath gently.
I am going to carry out an experiment to measure the change in mass of
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.
Remove the metal object from the first beaker and insert it into the second one.
Plan 1. Collect 4 different sized beakers 2. Boil some water in the kettle 3. Pour 50ml into each beaker 4. After 1 minute check temperature 5.
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
Obtain a sample of metal that has been immersed in boiling water and place it in the cup of water.
Quickly and carefully transfer the heated metal from the test tube to the water in the calorimeter.
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 a 100ml beaker 30mls of water was placed the temperature of the water was recorded. 1 teaspoon of Ammonium Nitrate was added to the water and stirred until dissolved. The temperature was then recorded again. This was to see the difference between the initial temperature and the final temperature.
3. Why are the crucible and lid heated at the beginning of the experiment before being weighed?