Lab Report: Pressure Temperature Volume

2. Obtained a 2-3 cm strip of magnesium metal ribbon and coiled it loosely into a small ball. Added the magnesium metal to the acid in the test tube.

During the immersion of the magnesium metal in the hydrochloric acid solution, white bubbles could be seen escaping the surface of the metal as gas was produced during the reaction. Depending on the temperature of the hydrochloric acid and the overall molar concentration, the rate of reaction differed but the same signs were shown. During the reaction between the magnesium metal and higher concentrations of hydrochloric acid, it was observed that the test tube grew quite warm to the touch. As the immersed magnesium strip sank down, it appeared coated in a layer of white bubbles that fizzed like a carbonated drink. In the lower concentrations of hydrochloric acid, the strip spent some time floating at the surface of the solution in the test tube, later sinking down to the bottom as the

Procedure: Have you made any changes to the procedure? Please explain. If you made no changes, state so. (1 point)

In this lab experiment our main focus was to get skillful in using tools such as the metric ruler, balances, thermometer, and graduated cylinder to capture measurements of length, mass, temperature and volume. Additionally, this lab helped us to become more familiar with the uncertainty of measurements, as well as becoming efficient with rounding our measurements to the correct numbers of significant figures. Our results are measured consistently with rounding to the closest answer we could possibly acquire as the data can tell you.

2. Read and record the temperature of the gas using the thermometer attached to the container.

About 80 mL of HCl was obtained and mixed with phenolphthalein. Using a LabQuest unit and Gas Pressure Sensor kit, the HCl mixture was added to the flask with the magnesium ribbon and allowed to react. When reaction was complete, the change of temperature and gas was recorded. This procedure was repeated for different masses of magnesium ribbon (masses found on page 89 of the lab manual). After the completed procedure, moles of H₂ produced in each trial were calculated. (The actual procedure can be found on pages 87-89 of the lab manual)

13. The temperature of the water was measured prior to the tube being placed in it and the temperature of the Hydrochloric Acid was measured after it 's temperature had adjusted.

I would use a bar graph because it would be easy to follow and understand the information presented.

After the twenty minutes elapsed, the flask was cooled to room temperature and then titrated with the remaining NaOH until the colorless solution remained pink. The final volume was then recorded. While solution #1 was heating the same process was repeated with solution#2 and the second burette

To start this experiment, set up the gas collecting apparatus. To start Part A, add approximately 15mL of distilled water to the test tube and record the temperature. Use about half of an Alka-Seltzer® tablet and record the mass. Close the test tube with the stopper with the tubing and tilt the test tube so the water and tablet react. When the reaction is finished, record the volume of CO2 recovered by lining the meniscus of the graduated cylinder up with the water level.

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

8.When the reaction is completed, record the volume of gas in the graduated cylinder. Record observations about which reactant was the limiting reactant.

n = number of moles. Using the equation R=pave/nt, the scientist uses their data to calculate the R with an actual R of 8.3 j/mol. Through this lab the scientist is using the chemical reaction of HCl acid and Water to create Hydrogen gas breaking down the magnesium finding the moles of magnesium in the container. This la focus on the properties of gas by using volume in liters and barometric pressure, which is the pressure exert by air in the atmosphere.

Experiment/Result/Analysis: In activity 17.8.1, we related volume and temperature, we had a empty beaker with air and a temperature probe in it, sealed with a rubber stopper that was connected to a syringe. We placed the beaker in cold water with a immersion heater and recorded the data on LoggerPro. As the water heated up, we observed that the pressure of the air remained constant because the temperature is also changing. We fit our data with a linear curve and concluded that the change in volume is directly proportional to the change in temperature.

b) An empty beaker was weighted. Then, water was filled in the beaker. The temperature was recorded at uniform intervals.