Solar Energy Lab Report

Step 3: Use the thermometer to identify and record the temperature for room temperature, in your refrigerator, in your freezer, and then research the temperature of boiling water (do not take this temperature) and record them in Table 2.

We took the plastic cup and added the stir bar into it, then we inserted the plastic cup and the stir bar into the styrofoam cup. Next, we secured the clamp on the ring stand rod, and then added the solution calorimeter to the other end of the clamp. Following that, we took the beaker and filled it with distilled water and transferred it to the graduated cylinder. Then we poured it into the plastic cup with the stir bar in it. We turned the stir plate to number 6 and let the water stir around for 10 seconds, then we added in our first effervescent tablet and let it for about a minute or until it was fully dissolved. We added an extra tablet to every test until we reached the total number of tablets we could insert which was 5. After we were finished with each test, we washed out plastic cup, the solution calorimeter, and the stir

Place the beaker on the hot plate, place the thermometer in the beaker and set the hot plate to 5oC.

Now, take the vial and place it into a laboratory drying oven. Leave it here for at least one hour to get the most accurate of results. After it is heated, place the vial into a desiccator to help bring it back down to room temperature. Finally, records its mass one last time. Keep placing the vial into the desiccator until the mass of the crystals and vile stops

9) Trial E: Remove the syringe and empty the beaker. Add a Thermometer to the beaker. Add 200 mL of Room Temperature water to the beaker and heat with a Bunsen Burner until it reaches 100° C. Remove the Bunsen Burner. Repeat Steps 5 & 6.

In this modern fast paced world that we live in, there are many issues that are looked over, energy is one of these. As a world, we are dependant on dwindling fossil fuel supplies and take for granted electricity, oil, and gas. There are four completely renewable sources of energy around us that should be used and developed, they are: wind, growing plants, flowing water, and the sun. These sources of energy are the ones we should be tapping, because they are reliable and renewable. Harnessing the suns energy is the most certain and ultimate energy source. Looking at a brief history and some facts about solar energy, a glimpse of the future can be seen, a future not dependant on

To begin the experiment, students first obtain a LabQuest with a temperature probe. First, you retrieve about 20gs of t-butyl alcohol and put it in a pre-massed test tube. Students then prepare one beaker with ice water and another beaker with warm water. Students will first put the t-butyl alcohol into warm water to prevent it from freezing in room temperature, and put the temperature probe in the test tube. Afterwards, students will place the test tube containing the t-butyl alcohol and put it in the ice water until the temperature begins to

7. Two minutes later, there was a layer of salt accumulated in the bottom of the beaker once the stirring was done, indicating the end of the experiment. 8. Steps five to seven were repeated except using the room temperature water. Data/Results: See the graphs/table Conclusion:

Third, we could try to keep the temperature of the water the same throughout the whole experiment, when we put 100°C water into a beaker, the temperature would quickly drop down maybe 10°C in a minute or so. So if we had a machine that would keep a consistent temperature the whole time, we could get a

Procedure: This lab starts off by making sure the logger pro and temperature probe are in proper condition. Then, the data collection must be adjusted to 15 minutes and 12 samples/ min. After that a Bunsen burner must be set up by assembling a ring-stand, ring, and wire gauze, and a crack-less beaker is used to boil some water. First the beaker and the large watch glass need to be weighed and the mass has to be recorded using a triple beam balance. Next, the beaker with 200g of ice is placed on the ring stand, and immediately heated over medium flame. An important note is to make sure the flame is perfectly adjusted so the ice does not melt on the counter while trying to adjust the flame. Furthermore, place the temperature probe in the ice so it is not resting at the bottom of the beaker, it is best to secure it with a small clamp. Additionally, click the green start button on the computer and stir continuously with a glass rod until the ice is completely melted. Once the ice has melted which is somewhere between 3-5 minutes, the stirring rate will slow

Rinse out beaker and dry it, preparing for next trial. Also reset stopwatch. Repeat steps 10-16 two more times until you have completed three trials in total. Measure the temperature of the hot water in celsius and record it to ensure consistency in temperature throughout the experiment.

Next get the three types of waters with the different temperature and measure 50ml of water. Take the thermometer and write down the temperature of the water . Then measure 4 grams of sugar of the balance with the wax paper. Then you are going to take the sugar and pour it in the hot water and immediately start the stopwatch and start timing the sugar dissolving. Stir with a straw until fully dissolved.

7.) Let the beaker sit on the hot plate for 3 minutes. 8.) Turn on the lab quest 9.) After a few moments put the temperature probe from the lab quest into the beaker.

After 6 hours, record your results and then throw the juice away. Medium Temperature (120 degrees Fahrenheit) 8. Fill a small metal pot about halfway with tap water. 9.

Introduction: Every chemical change is accompanied by a change in energy usually in the form of heat. If heat is evolved, the reaction is exothermic, and if heat is absorbed, the reaction is endothermic. The energy change of a reaction that occurs at constant pressure is called the heat of reaction or the enthalpy of reaction (ΔHr). This quantity of heat is measured experimentally by allowing the reaction to occur in a calorimeter. In this experiment you will determine the heat of neutralization when an acid and a base react to form 1 mole of water. In a perfect calorimeter, heat is exchanged only between the reaction and the calorimeters water. Technically, some heat may may be absorbed the calorimeter. All calorimeters exchange some heat with its environment. This amount of heat is called the calorimeters heat capacity (the amount of of heat required to raise its temperature 1∘Celsius). We are going to “pretend” that our calorimeter is the perfect calorimeter.