Thermal Energy Lab

Use ice if you need to. Then, fill one beaker with 175 mL of water and the other with 350 mL. Warm the water in the 350mL beaker up to 55 degrees celsius and cool the water in the 175mL beaker to 15 degrees celsius, the same temperature as the pitcher because it will be your control group. Once the beaker that should be heated is at 55 degrees celsius, pour 175 mL of the water into a glove and pour the other 175 mL into a ziplock baggie. Pour the 15 degrees celsius, 175 mL of water into another ziplock baggie. Before you set these in water, have a stopwatch ready and make sure that the water in the baggies and glove is at the right temperature.

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.

13. Calculate the change in temperature for the water caused by the addition of the aluminum by subtracting the initial temperature of the water from the

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

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.

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

Purpose: The purpose of this experiment was to find the specific heat of an unknown metal, the heat of a reaction, and the heat of neutralization. Conclusion: Concepts covered in the lab were using formulas to find changes in temperatures, the heat capacity of water, molar masses of a metal, the change in enthalpy for a reaction, and the heat of solution per gram of a solid sample. Therefore, we learned how to apply these concepts into given materials and instructions in order for us calculate the heat capacity of a metal sample and how heat (energy) affects the system depending on certain surroundings.

You want to first open and organized you tools that came in the cool blue light experiment kit that can be found here (http://www.scientificsonline.com/product/cool-blue-light-experiment-kit). You then gather your different temperatures of water. You can use a Keurig brewed hot water setting for boiling hot water which came out to a temperature of 210 °F or more. Then get a bottle of water that is room temperature around 72 °F. Now take took some ice cubes and put them in a cup while I cont setting up my supplies. you now want to set the cups up for the chemicals and label which cup would be cold, hot, and warm. The kit came with these tiny spoons to use in order to get the chemicals out. You will need to use 1 spoonful of luminol and perborate

Now determine the mass of the water using the difference. Place the thermometer in the water for 3 minutes, then read the temperature. After the metal has been in the water for 5 minutes, use the tongs to transfer it to the calorimeter. Stir the water and occasionally read the temperature without removing the thermometer.

Measure 80 mL of water in a graduated cylinder Step 6. Transfer the water into the small 150 mL beaker Step 7. Set the beaker of water on the stand Step 8. Measure the temp of the water without the thermometer touching the glass beaker Step 9. Set the chip under the stand and set it fire and let it

Use the retort stand (like in Step 6) to grab the thermometer and put the thermometer head (big red bit) into the water of the outer container. 10. Obtain the required amount hot water from a urn/kettle with another appropriately sized beaker and wearing a heatproof glove and pour it into the outer

Introduction: The purpose of this experiment was to examine the relationship between heat transfer, temperature, and specific heat capacity of water and a metal. Prior to beginning the experiment, it was known that specific heat is the amount of heat needed to raise the temperature of a given sample of substance one degree Celsius, and specific heat capacity is amount of heat needed to raise temperature of one kilogram of substance one degree Celsius. The formula to solve for specific heat capacity is: Cp = Q/ (m *ΔT) or Specific heat capacity =

We prepped for the experiment by turning on the hotplate and giving it time to heat up, putting water into a large beaker, plugging the temperature Probe into the computer, placing the rubber stopper into the Erlenmeyer flask, and connecting the pressure tube into the rubber stopper. Next, we used a ring stand to lower the Erlenmeyer flask into the water

Once the range is obtained, remove the thermometer and beaker. Pour out the hot water and allow both the thermometer and the beaker to cool. Once cool, repeat the previous steps with the second compound, tetradecanol. At the conclusion of the second experiment, repeat the steps for a third and final time using an equal mixture of both compounds. Be sure to record the melting point range for all three experiments.

Rinse the thermometer with tap water and dry. Insert the thermometer in the calorimeters top and measure the initial temperature of the base 28.2∘C