Lab 10 Carbonation Release Full Lab Report PDF

Preview

Summary

Download Lab 10 Carbonation Release Full Lab Report PDF

Description

Gas Changes Introduction: In this experiment that is performed a gas will be produced and the pressure will be recorded. Temperature will then come into equation once the pressure of the first part is completed. The Ideal Gas Law, which is given by the equation PV=nRT, involves pressure and temperature. The relationship is given between pressure, volume, temperature, and amount of moles of gas. Both pressure and temperature are directly proportional to each other and can be shown in this lab experiment. Methods: Part I: A sample of 0.201 g of sodium bicarbonate for the first trial was weighed out. This sodium bicarbonate was then transferred to a 250 mL Erlenmeyer flask. The flask was then sealed with a Luer lock that had two holes, one hole was for a pressure sensor and the other for a syringe. Acetic acid was measured and was 2.9 mL. The acetic acid was transferred to the syringe and we made sure that no extra air was trapped inside. The syringe was connected to the Luer lock, but it was not added immediately. The monitor was set up to collect data and then acetic acid was added. The acetic acid was swirled around in the flask. When it was mixed white fizzy bubbles were created and then it would turn back to liquid. The contents in the flask were disposed in a separate beaker to be disposed of later in the experiment. Another two trials were run the same way except with different amounts of sodium bicarbonate and acetic acid. For the second trial 0.15 g of sodium bicarbonate and 2.25 mL acetic acid were used. In the third trial 0.10 g of sodium bicarbonate and 1.55 mL of acetic acid were used. After the third trial we did not break the seal to dispose of the contents.

Part II: A 1 L beaker was used to prepare a water bath. We added water that filled about one third of the beaker. A temperature probe was then added to the LabQuest to monitor the water temperature. If the water was below 25 °C then we could submerge the flask in the water bath. Our water temperature was at 22.5 °C and we proceeded to submerge our flask from Part I. Once the pressure was recorded the water bath was slowly cooled down four more times by 5 °C intervals. The pressure in the laboratory was 99.38 kPa. Results: Table 1: Mass and Volume of Reagent Amounts and Pressure at 100 Seconds; Part 1 Trial

Sodium Bicarbonate Mass (g)

5% Acetic Acid (mL)

Max Pressure (kPa)

1

0.201 g

2.9 mL

117.73 kPa

2

0.15 g

2.25 mL

110.63 kPa

3

0.10 g

1.55 mL

106.44 kPa

Table 2: Temperature of Water Bath and Pressure of Flask; Part 2 Trials

Temperature (°C)

Pressure (kPa)

1

22.5 °C

107.99

2

17.5 °C

106.95

3

12.5 °C

105.08

4

7.5 °C

102.54

5

2.5 °C

101.60

Discussion: In this experiment we saw in the first part of the lab that carbon dioxide was formed from the sodium bicarbonate and acetic acid. The balanced equation can be shown by NaHCO3 +

HC2H3O2 → NaC2H3O2 + H2O + CO2 and we can see from this equation that what occurs is a double displacement reaction and then a decomposition reaction that results in carbon dioxide gas1. That is what can be seen from the observations when both the sodium bicarbonate and acetic acid are mixed together, the big fizzy bubbles is the CO2 gas forming. As mentioned earlier, we know that PV=nRT is the ideal gas law, which shows the relationship between pressure, volume, temperature, and moles of gas. This then leads to other equations such as Boyle’s law, Charle’s law, or Avogadro’s law. We can use the ideal gas law to derive other formulas to solve problems with different conditions2. In part two, it resulted in seeing how the ideal gas law relationship works. The law mathematically states that pressure and temperature, temperature and volume, pressure and moles of gas, and volume and moles of gas are all directly proportional except for pressure and volume3. It is shown from cooling the water bath that the pressure and temperature remain linear. The temperature decreases by increments and the pressure also drops down with it. Conclusion: There are various gas laws that can be derived from the ideal gas law. This formula is very helpful if at least three of the variables are given. It is shown here in this experiment the proportional and nonproportional conditions of this law, showing that the ideal gas law is accurate and reliable. References: 1. Helmenstine, A. M. Know the Equation for the Baking Soda and Vinegar Reaction. https://www.thoughtco.com/equation-for-the-reaction-of-baking-soda-and-vinegar-60404 2. Interactive General Chemistry (Atoms First). (2019). [ebook] Macmillan. Available at: https://macmillan.vitalsource.com/#/books/9781319263744/cfi/6/416!/4/2/8/16/2@0:54.9

3. http://www.sussexvt.k12.de.us/science/Kinetics/Gas Laws.htm....