Specific Heat Capacity Lab

Ø Then I will record the temperature of the water in the calorimeter, using a thermometer to give a good degree of accuracy.

If 10.0g of solid baking soda is poured into 30 mL of citric acid, then a reaction will occur and an increase in temperature will be observed. Whereas, if a piece of magnesium metal is added to 30 mL of Hydrochloric Acid, then a reaction will occur and an increase in temperature will be observable. For Part 3 of the experiment, if 50 mL of tap water is placed in a can 2.5 cm inches above a burning marshmallow, then through the process of calorimetry the energy content of the marshmallow should be 5.0kJ/g (the value provided by the United States Department of Agriculture).

Fulfilling the purpose, after concluding this experiment, the formula of an unknown hydrate was able to be identified. In order to obtain the data needed to develop a response to the purpose, multiple measurements were collected. The mass of an evaporating dish was measured without copper (II) sulfate hydrate (before and after heating), then measured with copper (II) sulfate hydrate before heating and with anhydrous after heating. Initially, the mass of an evaporating dish was recorded, then the dish was heated and the mass was again recorded. Through this additional step of heating, it insured that no excess water remained in the dish which, as a result, would alter the data. Copper (II) sulfate hydrate was added to the dish and the mass was

Also, in this lab we explored the thermoregulation strategies and determined the effectiveness of each strategy. In this exercise, we recorded the temperature of the back of our hand before and after placing it into an ice bath. Before

The purpose of this experiment was to find the specific heat of zinc (Zn) metal. This was done performing the experiment. Using a coffee cup calorimeter filled with water you took the temperature of the water both before and after it was placed into the calorimeter. After taking the metal out it was massed.

In this experiment, a scientist will test which of three metals copper, steel, or brass produces the most thermal energy. The independent variables are the three metals used and the time amount of time the metals spent in water. The dependent variable is the thermal energy conducted. The control for this experiment would be a nonconductive material and the constant materials are the pot, stove and Styrofoam cups used. The data will all be calculated in degrees Fahrenheit.

This property of Magnesium explains why it could produce a higher temperature when combined with

The purpose of this laboratory experiment was to compile data enabling students to classify compounds as ionic or covalent. To do this, students tested the compounds: sodium chloride, calcium chloride, potassium chloride, sucrose, salicylic acid, wax, and stearic acid through their conductivity, solubility, and recorded the order of which the compounds melted. Conductivity was tested by using two paper clips placed in the compounds that were located in water and observing if they were able to charge a closed circuit. Solubility was tested through placing small amounts of the compounds into test tubes and dissolving them with water and the process was repeated with ethanol. The results from this experiment was that the compounds: Sodium Chloride,

After a further analysis of the results it has been seen that the averages of the results have proven the hypothesis to be correct. Hence the constructed calorimeter has been more efficient in reducing the enthalpy number upon burning ethanol compared to the copper calorimeters that have been previously used. Its has become known that due to more heat being absorbed the enthalpy number has significantly been improved by almost 10%.

In this lab, we will be learning about endothermic reactions and exothermic reactions through experiments involving temperature probes. The first reaction we will be performing involves citric acid and baking soda, and the second reaction involves magnesium metal hydrochloric acid. The two reactions for this are:

Materials were gathered and the mass of a calorimeter was measured, then HCl was poured into the calorimeter and the mass was measured again. A 7 cm magnesium ribbon strip was cut into two parts, approximately 4 cm and 3 cm, respectively. The temperature of the HCl was recorded, then the 3 cm magnesium strip was added to the solution and the temperature was measured again. Another trial was conducted with the 4 cm strip after the disposal of the first mixture.

5) During calculations, the specific heat capacity of the copper calorimeter was not included. This is

The heat of combustion produced increases the temperature of the calorimeter system. About 10 to 15 minutes after ignition the heat exchange between the calorimeter bomb and the water surrounding it in the inner vessel is completed. The temperature rise is then measured and serves to calculate the gross calorific value Ho. This calculation is possible only if under the same test conditions the heat capacity C of the adiabatic system has been determined previously by burning a reference

A common example of heat of fusion is when ice is melted to water. The manufacturing of United States monetary coins requires use of the heat of fusion process. For example, in making pennies, solid zinc and copper metals are placed into a furnace and heated by the heat of fusion process until they are

The purpose or aim of this investigation is to explore and compare the melting points and boiling points of primary, secondary, and