Calorimetry Lab

After each of the solids were completely dry, each was placed into a MelTemp device. The temperature at which each solid began to melt and completed melting was recorded.

The purpose of this experiment was to determine the heat of combustion of magnesium using Hess’s Law. This experiment was significant in understanding how heat can be absorbed or released and how using a calorimeter can help measure heat flow. Part A of this experiment used two dry Styrofoam cups and a magnetic stir bar to create a calorimeter. Temperature was measured and distilled water was placed into the calorimeter, and after 2-3 minutes, boiling water was mixed in. The computer continued to take data for 6 minutes and then the calorimeter was reweighed and emptied. Part B and C were the same, only using two different types of magnesium (magnesium ribbon (part B) and magnesium oxide (part c)) instead of the boiling water. The major result is that all of these experiments release energy because the calorimeter temperature increased.

Then 8.0g of copper sulfate crystals were placed inside the beaker and the mass was recorded for the actual crystals. 50 mL of water was added to the beaker with the crystals. The ring stand was set up with the wire mesh on it and one partner should place the mixture in the beaker on it should be heated without letting the mixture boil. Stir the mixture and heat until the crystals are dissolved. While one partner does this, the other should obtain 1.5g of iron filings in a measuring cup and records the mass. Then the iron filings should be added small amounts at a time to the heated solution. Stir continuously until all the mixture is added to the beaker. Then it sat for 10 minutes and observations were recorded. Record the mass of a filter paper and set up a filtration apparatus with the filter paper in a funnel over an Erlenmeyer flask. Decant the liquid through the paper slowly trying not to allow any solid to get on the filter paper. Then with de-ionized water, rinse your solid in the beaker and let the solid settle then decant the liquid. Repeat the washing twice more and in the last time guide all the solid into the filter paper. Then place the filter paper on a watch glass and then into a warm oven to dry. After it is cool, record the mass of the watch glass, filter paper and solid. If there is not enough time to cool, you may have to do it the next

For q, you found how much heat was gained by the water so you know that same amount of heat was lost by the metal. Therefore, qmetal = -qwater. The mass of the sample was recorded from the baggie. The temperature change

After performing the experiment, the results were that copper pennies have a greater density and mass than the zinc pennies. These results supported my hypothesis of since copper has a greater density than zinc, then the copper pennies will have a greater mass than the zinc pennies. Some errors that occurred during this experiment are the non-precise measurement of the water and how some of the copper pennies had grime on them because they were old. This extra grime caused the mass of the pennies greater. A precise measurement of 15 mL of water and clean copper pennies would improve the experiment and the amount of errors would be

Abstract: This experiment introduced the student to lab techniques and measurements. It started with measuring length. An example of this would be the length of a nickel, which is 2cm. The next part of the experiment was measuring temperature. I found that water boils around 95ºC at 6600ft. Ice also has a significant effect on the temperature of water from the tap. Ice dropped the temperature about 15ºC. Volumetric measurements were the basis of the 3rd part of the experiment. It was displayed during this experiment that a pipet holds about 4mL and that there are approximately 27 drops/mL from a short stem pipet. Part 4 introduced the student to measuring

The filter paper should be left out overnight to dry out since all the water mass will turn into water vapor and separate from the CuO. Then scape the filter paper to get all the CuO off for it to react with excess amount of sulfuric acid, H2SO4 because the copper has to be the limiting reactant in order to get the total mass of the copper. (CuO (s) + H2SO4 (aq) -> CuSO4 (aq) + H2O (l)). Now add 0.1 g of zinc filings to the beaker and stir until the solution is colorless because originally the solution was blue from the Cu2+ so for the solution to be colorless that means all the copper has turned into a solid and all by itself (CuSO4 (aq) +Zn (s) -> Cu (s) + ZnSO4 (aq)). Finally, the solution must be filtered again to separate the copper from the ZnSO4 and the filter paper is left to dry again. The mass of the filter paper and the watch glass mass was taken beforehand again to later on subtract these measurements from the mass of the copper. The mass of the copper was weighed once the paper was all dried up and what was left was the

During the heating period, a noticeable change took place in the sugar test tube – it began to caramelize, melting into a golden brown color, then finally a dark brownish/black hue; it remained constant at that color. The copper sulfate began losing color when applied to the heat, turning from a bright blue to white and remained white after heating. Once cooled, 2-3 drops of water were added to each tube; the sugar remained the same, while the copper sulfate immediately bubbled and transformed from white back to its original blue hue. Next 1-3 grams of the hydrated copper sulfate were added to a crucible, which was weighed prior to adding the sample, then heated gently with a Bunsen burner. Once the salt stopped changing color, it was heated for an additional 5 minutes, then the total mass was measured. Finally, a pea-sized amount of Epsom Salt was added to a test tube and heated for 1 minute without the tube becoming red

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).

First, each metal’s description and weight was recorded. Additionally, the weights of each cylinder used was recorded. Next, a graduated cylinder was filled with 20mL of water and unknown metal II was fully submerged in the water 3 times. Each time, the volumes were recorded and the difference between the final volume and initial volume was calculated. This test was repeated for unknown metal IV.

When the water in the beaker has boiled for 10 minutes, pour the metal into the Styrofoam cup, and take the temperature, recording the highest one. Drain the water and remove and dry off the metal. III. Data: Trial 1 2 3 4 Mass of metal #8 60.33g

50mL of 2M NaOH was added to the two stacked Styrofoam cups in a 400mL beaker. The cup was then covered with a plastic lid and a temperature probe was inserted through the lid and into cup in a way so that it did not touch the bottom. 3-4 temperature readings were then collected by clicking “collect” on LabQuest to start Run 2, and initial temperature was determined. 50mL of 2M NH4Cl was then added to the NaOH solution in the cup and swirled around. The rest was repeated from the first

The purpose of this lab was to calculate the percent of water mass the copper (II)

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

3. When the flasks are removed from the hot water bath filled with water vapor and then cooled. Once the flask is cooled and vapor condenses in the flaks the reported molar mass of the liquid will remain unaffected since the water vapor in the flask is the same when changing from heating to