Can The Specific Heat Of An Unknown Metal Be Found Using Calorimetry

The temperature probe was kept in the calorimeter until the temperature had been stabilized and was calibrated. A beaker was placed on a hot plate with dial turned between three and four. Another 100.00 ml of deionized water was added while the beaker is heating up. Using the temperature probe, the beaker was measured

We started by putting 100 mL of water into a coffee cup calorimeter (a polystyrene cup inside another polystyrene cup as an insulator), a magnetic stir bar was added and using the program LabProTM the

Then an estimated (by trial and error) 1-3 grams of hydrated copper sulfate was added to a crucible with the lid on top. The total mass of the hydrated copper sulfate was recorded by subtracting the total mass of the crucible, lid, and sample from the mass of the crucible and lid (described in table 1.3). By attaching the wire triangle to the ring, the crucible was able to sit securely while having the bunsen burner underneath. Lighting the burner once again, each substance was heated for several minutes until estimated that the compound had changed color. Once a prevalent color change had been observed at approximately 4 minutes (blue green color) the crucible was set on the counter using the tongs to cool for approximately 5 minutes.

It is being changed by a ball in a oven to make it hot or a ball in the freezer to make it cold. Temperature can be measured by

Firing to Red Heat - the process of putting a substance in a crucible and heating it until it glows red. c. Heating to Constant Mass - the action of heating a substance until the mass remains constant. d. Molecular Formula - the true formula of a compound, a multiple of the empirical formula e. Massing by Difference - An indirect manner of finding the mass of a substance, through finding the difference between a container and the container holding the substance Crucible tongs are used to pick up crucibles after heating and before massing because the crucible is typically too too hot to handle with hands. The suggested times for heating and cooling are very important in order for there to be no error in calculation when handling the metal.

Continue to heat the solution until it reaches about 55℃. Using the test tube holder, transfer the liquefied solution tube to the 25℃ water and record the temperature at 30-second intervals using a clock or stopwatch using a pencil until the solution reaches 35℃ or close to the temperature due to experimental error. While cooling, gently stir the solution using the thermometer until the solution begins to solidify. Once all the data is collected, reheat the solid solution tube in the warm water until it melts and remove the thermometer and wipe it off to avoid the solution adhering to the thermometer. After the data has been recorded, clean-up the lab station and put away the lab

Before starting the heating process, measure the weight of the crucible with its cover first and then tare the balance, and after that adding about 1 gram of the sample to the crucible with its cover, and then weigh it. Moreover, it is possible liberating harmful gases during the process of heating; therefore, being careful is important. The heating process ends when this sample changes the color to brown because water of hydration is removed to the sample. Additionally, give time to the small cool down and measure its weight. Next, transfer the sample to a 50 mL beaker and mixes with distilled water, which gets by rinsing the crucible with its cover in 8mL, so the solution is generated.

Materials and Methods The chemicals used to perform this experiment were distilled water, sodium chloride (NaCl), ice,

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.

In this graph the results is about what we expected, which is a big amount of heat given off. In observing the graph the distance between reaction 1 and reaction 2 shows the total amount of heat given off which is the combination of 1&2 in comparison to room temperature that the water was originally at. Through the experiment there was a lot of question as to if we were doing it right, were we swirling the solution around enough, did we open the top right so heat would not escape, did we collect the data at the right time? Now looking back I see that many of the things that our group did defiantly altered our data, making me question the reliability of the data we collected. The first reaction was CaCO3(s) + 2HCL(aq)------- CaCl2(aq) + H20(l) + CO2(g) and the second reaction that was given was Ca(OH)2(s) + 2HCl(aq)-------CaCl2(aq) + 2H2o(l) combined gave off about 57 degrees Celsius going into a system (Calomitery and Hess’s Law).

In this experimentation, the data showed that the 70% melted the fastest. It melted in three minutes and ten seconds and has a melting point of 54.2℃. The 90% melted the

Introduction: In this lab, of water in a hydrate, or a substance whose crystalline structure is bound to water molecules by weak bonds, is determined by heating up a small sample of it. By heating, the water of hydration, or bound water, is removed, leaving only what is called an anhydrous compound. Based on the percent water in the hydrate, it can be classified as one of three types: BaCl2O ⋅ 2H20, with a percent water of about 14.57%, CuSO4

The solid model Fig 2. The solid model split into hexagonal patterned circles for applying heat load The top face of the Fig 1 is heated by Laser. The top surface of another model has a hexagonal patterned six circles and one circle at the centre as shown in Fig 2. The heat flux is non- uniform over that face.

Calorimeter helped many generations to measure the quantity of heat using different types of devices; also they followed a specific procedure and equations to find out quantitative

After two minutes, determine the temperature of the tap water, this will be the initial temperature in the equation Write out constants for the equation -q(exo)=q(endo) Fill the same graduated cylinder this time with 40mL of tap water Pour the 30mL of tap water into a second styrofoam cup and mark with a pencil the water level in the cup Pour the 30mL of tap water out and fill the same styrofoam cup with hot water using the pencil mark as a guide—be careful not to spill hot water or touch hot surfaces Quickly mix the 30mL of hot water to the 60mL of tap water together in a third styrofoam cup Measure the temperature of the combined hot/tap water mixture, this will be the final temperature in the equation Calculate the equation with the temperatures found with the thermometer Independent Variable: ratio of water samples in mL Dependent Variable: The temperature of the hot water Controlled: using the same hot water (coffee pot), styrofoam cups, and thermometer