Part A
Procedures Observations
1. Put 400 mL of tap water into a beaker. Heat it on a hot plate until it starts to boil.
2. Put a rubber-stopper assembly into a 125 mL Erlenmeyer flask. Twist the stopper into the flask's neck until it is tightly secured. Connect the connector and the gas pressure sensor valve, then twist in a clockwise motion. Prevent gas leakage by covering the stopper and flask's top with parafilm. Twist the white valve until it is perpendicular to the valve stem in order to close the two-way valve.
3. Use a syringe to collect 3.0 mL ethanol (EtOH). Twist the syringe so that it attaches to the two-way valve. Wait until the TA instructs you to put the flask into the water bath.
4. Using LabQuest2, connect the temperature
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probe to CH 1. Connect the pressure sensor to CH 2. ("Graph --> graph options --> change x axis to temperature. Graph 2 --> y axis --> unselect ch1:temperature. click ok." "Mode --> selected events --> OK" "ch2:pressure --> change units --> mmHg") 5.
Record air pressure (mmHg) in the Erlenmeyer flask without solution. ("should be ~760 mmHg") Hold the temperature probe up in the air and record room temperature (°C). Observations: refer to table 1. (data table of °C temperatures)
6. Twist the white valve until it lines up with the valve stem in order to open the two-way valve. Push the syringe's plunger in order to transfer the EtOH into the flask. Immediately twist the white valve until it is perpendicular to the valve stem in order to close the two-way valve. Twist the syringe in a counter-clockwise direction in order to remove it from the two-way
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valve. 7.
Use LabQuest2 to record pressures and temperatures. (press green play button) Once pressure and temperature measurements stop changing, keep the data. Record the vapor pressure of the flask with ethanol at room temperature.
8. Put the closed flask into a water bath at room temperature in a 1 L beaker. Ensure that the entire flask is covered. If the flask begins to float, clamp it down. Put the temperature probe in the water bath. Using a pipet, add some boiling water from the hot plate to the water bath until the temperature of the water bath increases by 3 °C. Use the temperature probe to stir the water bath. Once pressure and temperature measurements stop changing, keep the data. Record the air pressure and vapor pressure for this temperature.
9. Repeat step #8. Using a pipet, add small amounts of boiling water from the hot plate to the water bath and collect pressure and temperature data. For each new temperature, record the air pressure and vapor pressure. Continue until you have gathered 6 measurements that range from room temperature to 40 °C.
10. Point the flask away from everyone and open the two-way valve in order to release pressure from the flask. Remove the stopper assembly, then fill up the flask with water. Discard of the solution in the sink.
Part
B Procedures Observations 1. Using the same Erlenmeyer flask as earlier, create solution 1. Add 1.0 mL of ethylene glycol to the flask, cover the flask, then add 2.0 mL of ethanol. Record the volume of ethylene glycol and the flask's pressure. 2. Using the same Erlenmeyer flask as earlier, create solution 2. Add 0.250 g of benzoic acid, cover the flask, then add 2.9 mL of ethanol. Swirl the flask around until the solute has fully dissolved. Record the mass of benzoic acid and the flask's pressure. 3. Using the same Erlenmeyer flask as earlier, create solution 3. Add 0.250 g of lauric acid, cover the flask, then add 2.9 mL of ethanol. Swirl the flask around until the solute has fully dissolved. Record the mass of lauric acid and the flask's pressure. 4. Discard of the solutions in the appropriate bottles in the fume hood. 5. Gather other students' data. 6. Delete your email and password from LabQuest2, then shut it down.
First, 100 mL of regular deionized water was measured using a 100 mL graduated cylinder. This water was then poured into the styrofoam cup that will be used to gather the hot water later. The water level was then marked using a pen on the inside of the cup. The water was then dumped out, and the cup was dried. Next, 100 mL of regular deionized water was measured using a 100 mL graduated cylinder, and the fish tank thermometer was placed in the water. Once the temperature was stabilizing in the graduated cylinder, the marked styrofoam cup was filled to the mark with hot water. Quickly, the temperature of the regular water was recorded immediately before it was poured into the styrofoam cup. The regular/hot water was mixed for a couple seconds, and the fish tank thermometer was then submerged into the water. After approximately 30 seconds, the temperature of the mixture leveled out, and was recorded. This was repeated three
Start with the hot water and first measure the temperature. Record it. 8. Then pour 40 ml into the beaker. You can measure how much water was used by looking at the meniscus.
When the liquid level is above the calibration line on the pipette, remove the bulb quickly and put your thumb or index finger over the pipette. Carefully “roll” finger to the side and allow the liquid to drop until the meniscus is level with the mark. Then hold the pipette over the flask to receive the liquid and remove the finger. Allow the liquid to drain out.
Tubing to connect flask to gas collection set up 1000 mL graduated cylinder Gas collection box Baking soda Vinegar Water Balance Scoop Procedure 1.Mass out desired amount of baking soda.
5.) One at a time, place your test tubes in the water bath and heat the first test tube to 25 , the second to 50 , the third to 75, and the last to 100 degrees c. Remeber to stir with your stirring rod every so often.
We must first begin the today’s lab by connecting the thermometer that digitally detects surrounding temperature to the Lab Pro Interface located on the computer via...
With the LabQuest device in hand, we then attached the Gas Pressure Sensor to channel 1, and the Temperature Probe to channel 2. The group then retrieved the rubber stopper assembly and attached the end of the tubing to the open stem of the Gas Pressure Sensor while leaving the valve stem in the open position. To hold the flask down in the water bath, we placed the glass stir rod into the opening of the rubber-stopper assembly and then insert the assemble into the neck of the 125 mL Erlenmeyer flask with a twist to make sure of a snug fit. We then closed the 2-way valve. Using the thermometer holder, we attached the glass stir rod at the base next to the rubber stopper, and placed the flask into the ice bath. Our group then fastened the thermometer to the ring stand. After procuring the 3-prong clamp we used it to hold the temperature probe away from all sides of the glass while keeping the probe submerged several inches deep. The group then placed the flask and assembly onto a hot-plate and recorded temperature and pressure data. We then turned the hot plate on and start recording data at 15 degree intervals until boiling occurred.
First of all, the purpose of this lab was to determine the water’s vapor pressure at different temperatures as well as to measure the molar heat of vaporization of water using the Clausias Clapeyron equation. The first concept out of many represented in this lab is the ideal gas law. The ideal gas law is used to get the number of moles of air trapped in the 10 mL graduated cylinder. Once we cooled the system so that water vapor is extremely minute, and then we determined the number of moles of air using the ideal gas law. The number of moles of air equals to the pressure (in atm) times volume divided by constant times temperature. One would assume that when the water is heated to 80 degrees, the number of air molecules in the air bubble would decrease, but it actually stays constant. This is due to the fact that there is no air coming in or out of the cylinder. As the temperature gets closer to 80 degrees, the number of air molecules stays the same but the water vapor increases. And the bubble expands to keep the pressure at the same level. The ideal gas law was also used when the partial pressure of air in the gas mixture is calculated. This is gotten from number of moles multiplied by the constant and the constant and the whole thing divided by the volume.
In a Styrofoam cup, record the temperature of the 200 ml of cold water. This is 200 g of water, as the density of water is 1 g/ml.
After the water, has been boiling for 10 minutes, and the temperature inside the test tube has been stable for 5 minutes, record the temperature and remove the thermometer.
Now, assemble and arrange all of the needed supplies so that they are easily accessible. Connect the IV tubing to the solution bag and allow the fluid in the bag to run through the entire length of the tubing, also known as priming the tubing. When this is done, clamp the tubing closed. You will then need to tear several pieces of tape, six to eight inche...
2. In the large beaker, put water and boil it completely. After that, remove the beaker from heat. 3. Sample tubes (A-D) should be labeled and capped tightly.
In a 250ml beaker place 100mls of water, measure the temperature of the water and record this initial temperature onto a table. Set the timer and add one teaspoon of Ammonium Nitrate to the water, stir this continuously until the Ammonium Nitrate has dissolved. After 1 minute measure the temperature and record it, do this for a further 2 minutes (3 minutes in total). Repeat this process for a total of 10 teaspoons.
The last part of experiment 5, was learning about specific gravity and temperature. Specific gravity does not have any units, it is unitless. When measuring for the temperature, we used a thermometer to calculate the Celsius of the water, 10% sodium chloride, and isopropyl alcohol. The specific gravity uses a hydrometer to measure the gravity of the liquids. Using the hydrometer, to figure out the measurements we have to look at it from top to bottom. The water for specific gravity was .998 while the temperature of it was 24
Our project for the unit 2 test will be a candle and water demonstration. This will show the different relationships between temperature, pressure, and volume.