Purpose/ Research Question: Determine the specific heat capacity of two unknown metals. Find two Ionic compounds out of the several given chemicals that would synthesize in the product of the most effective hand warmer. Hypothesis: For both metals one and two, we can calculate the specific heat capacity within five percent error. The ideal hand warmer for cost, toxicity, and heat given off would include 5.0 g Magnesium Sulfate (MgSO4) and 10 mL of deionized water. Procedures: We set up an appropriate apparatus including a Styrofoam calorimeter cup containing room temperature deionized water, two thermometers, and a clean beaker also containing deionized water directly on a heat source. After heating up the water until its boiling point, we recorded the mass of each metal and carefully placed the selected metal inside the boiling water until the temperature of the water containing the metal was constant. Quickly, we placed the hot metal from the boiling water in the calorimeter cup containing room temperature water …show more content…
We calculated the specific heat of metal one to be 0.39 J/g℃ which correlates to the exact specific heat capacity of element 30 Zinc. For metal two, we calculated the specific heat capacity to be 0.38 J/g℃ which was close to the actual specific heat of element 23 Iron. The specific heat capacity of Iron was 0.45 J/g℃. Our inaccuracy could be a result of not reading the thermometer as accurately as we could have. To improve yield in the future, we could make sure we record more accurate temperatures. I also accept my hypothesis on the most effective hand warmer. In terms of heat given off, toxicity, and price, Magnesium Sulfate was indeed the best choice for a hand warmer because when compared to the other given chemicals, it was the most exothermic in water, it is relatively nontoxic, and is very
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