Chemistry Lab Report
Determining Best Calorimeter
Dylan Mendonca
12-B
Background: Calorimetry is the science of measuring the heat of chemical reactions or physical changes. Calorimetry is performed with a calorimeter. A calorimeter can be any container from a cup to a Calorimeters need to be well insulated as calorimetry relies on the fact that temperature change only occurs within the solution and that no heat escapes to the surroundings. That is why it is important that calorimeters are well insulated. However, heat loss cannot be avoided so scientists, when conducting experiments, need to choose the calorimeter that allows least heat energy to escape, therefore, retaining as much heat within the solution
Research Question: By
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Only keep a pen and paper away from the experiment to record results
Procedure:
1. Rinse both measuring cylinders with distilled water then rinse one measuring cylinder with hydrochloric acid (HCl) and another with sodium hydroxide (NaOH) 2. Using one of the disposable pipettes, measure 40cm3 of NaOH (1.0M) in the measuring cylinder you rinsed with NaOH and pour this into Calorimeter #1 (Glass Beaker). Place thermometer inside solution 3. Using the other disposable pipette, measure 40 cm3 of HCl (1.0M) in the other measuring cylinder 4. Now record initial temperature of NaOH on the thermometer 5. Add the 40cm3 of HCl to the NaOH solution, close the calorimeter with the lid (making sure that the thermometer sticks through the hole) and start the stopwatch 6. Since the reaction is very quick, record the temperature every 5 seconds for 45 seconds. If the temperature doesn’t reach a stable value after 45 seconds, continue to take readings of temperature 7. Wash glass beaker with distilled water and repeat steps 1-6 with same calorimeter 2 more times 8. Repeat steps 1-7 with Calorimeter #2 (Styrofoam Cup) and Calorimeter #3 (Copper Cup)
Table 1 – Raw and Processed Data from Experiment for Calorimeter #1: Time (s) | Temperature (°C) (±0.5°C) | Average Temperature (°C) (±0.5°C)
29. When the thermometer reads 40°C, carry the beaker out of the heating apparatus with a beaker tong.
11. The experiment was repeated three more times using different water temperatures (room temp water, cold temp water, hot temp water).
2) Heat one to about 50˚C, and place other one in calorimeter (at around 20˚C)
Place the beaker on the hot plate, place the thermometer in the beaker and set the hot plate to 5oC.
4.Measure 35mL of warm water and add them into each of the 4 test tubes at about roughly the same time. It is essential that the water is warm. Do not seal the test tube.
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.
Task 1 Hypothesis By increasing the mass of substance using 20ml of water starting at room temperature there will be 10oc change, either an exothermic change or an endothermic change. Aim The aim of this investigation experiment is to find out what mass of substance is required for an exothermic or endothermic substance to achieve a 10oc temperature change. Set objectives • 7 masses of each substance should be used in this experiment: 0g, 0.25g, 0.50g, 0.75g, 1.00g, 1.25g, 1.50g, 1.75g, and 2.00g. • Measure the start and end temperature for each substance using a thermometer.
First, get a hot plate and scale, and plugged them in, and turned them on. Then, get a thermometer to measure the temperature of the water. Then, get a 25 ML beaker. After that, measure the beaker on the scale before adding water. Then, fill the beaker up with water and measured it. After, add 6 scoops
Insert a thermometer into the designated hole on the lid, and into the water chamber opening.
The temperature of the product was monitored. The product was observed for one minute. At station 8, the temperatures of the HCl and sodium hydroxide (NaOH) were measured. Five milliliters of NaOH were placed in the test tube. Five milliliters of HCl were added to the test tube.
Slide the vial into the water in the calorimeter and place the lid on top. Stir the water and continue recording temperature versus the time for a minimum of 20 minutes. If the rate of cooling remains constant for 7 minutes and the temperature is at least 2.5 degrees celsius below the maximum recording, recording can be stopped. Remove the temperature probe and vial. Dry the vial and record the mass of the vial with the lid and the
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
The initial temperature of the water was recorded with a thermometer so a change in temperature could be determined. This probe was then placed in the sandwich bag while sealed to observe the temperature inside the assumed calorimeter.
Use the measuring cylinder to get 1.5ml water and pour it into a test tube
Compare the experimental results obtained from the hand-held thermometer and the digital prove with the theoretical overall enthalpy of solution.