Carbonation Release Lab Report

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Feb 20, 2024

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Carbonation Release Lab Report Megan Salyer – Section 11 Title: Carbonation Release: Testing the Ideal Gas Law Introduction: In a chemical reaction when gas is produced, the pressure of a reaction will change based on the amount of gas being produced. The relationship between pressure, volume, temperature, and the amount of gas is explained by the ideal gas law, PV = nRT. P represents pressure in atmospheres, V is volume in liters, R is the universal gas constant, 0.0208 L atm mol -1 K -1 ) and T is temperature in Kelvins. The idea of this experiment is to understand the change of a gas and its properties that happen when variables, such as temperature, is manipulated. I hypothesize that the temperature and pressure are directly proportional to each other, because the temperature is held at a constant indicated by Boyles Law. Methods: To begin the experiment, we set up a 250 mL Erlenmeyer flask and set up a pressure sensor to the LabQuest monitor to record the pressure changes during the reaction. We obtained .238 g of sodium bicarbonate and put it into the Erlenmeyer flask. We then obtained 3.0 mL of acetic acid in our syringe, ensuring there was no excess air to mess with the pressure. We sealed the flask with the rubber stopper and luer lock connections. We added our 3.0 mL of acetic acid from the syringe to the Erlenmeyer flask. We had our LabQuest run and take 10 samples for 200 seconds. Once the pressure leveled out and stopped increasing, we disposed of the waste properly and rinsed the flask with DI water. We repeated the exact same process for trials two and three. However, in trial two, we used .164 g of sodium bicarbonate and 2.3 mL of acetic acid. In trial three, we used .109 g of sodium bicarbonate and 1.6 mL of acetic acid. The only difference was in that in trial three, we did not break the seal and remove the stopper. Instead, we prepared an ambient temperature water bath in a 1 L beaker with a temperature probe inside of it. We connected the temperature probe to the LabQuest. We submerged the flask into the water bath, recording the temperature and the pressure from LabQuest. We repeated this four times changing one thing: the temperature of the water. We added ice into the water, steadily decreasing it from about 25 degrees Celsius to 0 degree Celsius. We recorded the temperature and pressure each time, monitoring the relationship between temperature and pressure. After completing these trials, we rinsed out the flask with DI water and disposed of our waste properly. Results: My results demonstrated that the increasing reactants has a direct relationship with gas production. The more reactant is used, the more gas is produced. This is evident in part one and trial one where we used the greatest amount of sodium bicarbonate, .238 g, and acetic acid, 3.0 mL. The pressure in trial one was 103.34 kPa. In trial three, we used the least amount of sodium bicarbonate, .109 g, and acetic acid, 1.6 mL. The pressure in this trial was 98.57 kPa. In part two, it is evident that the temperature and pressure have a direct relationship. As we decreased the temperature of the water and submerged the flask in it, the pressure inside of the flask decreased. In trial one, when the water temperature was 13.5 degrees Celsius, the pressure was 96.33 kPa. In our last trial, when the water temperature was 1.0 degree Celsius, the pressure was 91.79 kPa.

It steadily decreased through the trials. This displayed that as temperature decreases, pressure does too. Figures/Tables: Part I: Peak Pressure (kPa) Trial 1 103.35 Trial 2 99.07 Trial 3 98.57 98 99 100 101 102 103 104 0 0.05 0.1 0.15 0.2 0.25 Mass of Reactants vs. Pressure Peak Pressure (kPa) Mass of Sodium Bicarbonate (g) Part II: Temperature (C) Pressure (kPa) Initial Reading 21.1 103.00 Reading 1 13.5 96.33 Reading 2 9.2 93.91 Reading 3 6.7 93.43 Reading 4 1.0 91.79

0 5 10 15 20 25 86 88 90 92 94 96 98 100 102 104 Temperature vs. Pressure Temperature (C) Pressure (kPa) Analysis/Discussion: In part one of this experiment, we combined sodium bicarbonate with 5% acetic acid to make a product. This equation for this reaction is NaHCO 3 (aq) + CH 3 COOH(aq) → H 2 O(l) + CO 2 (g). We observed the carbon dioxide bubble up and get released into the air. This happened because this reaction is a neutralization reaction, where sodium bicarbonate is being neutralized by acetic acid. As we increased the number of reactants used in the equation, the pressure increased. Pressure and number of reactants have a directly proportionally relationship (Hart). In trial three, where we had the most reactants., .238 g of sodium carbonate and 3.0 mL of acetic acid. This experiment demonstrates the ideal gas law, PV = nRT, which defines the relationship between volume, temperature, and pressure. In part two, we saw the directly proportional relationship between temperature and pressure. When we placed the Erlenmeyer flask in room temperature water, the pressure was much higher than when we placed the flask in ice cold water. This can be explained in Gay Lussacs Law, which states that a gas pressure is proportional to temperature when it is held at a constant volume (Millero). In this experiment, this was proven true. Conclusion: In part one, we found that the more moles of reactants present in their reaction, the higher the pressure. This is because the particles were packed more tightly together, which causes the pressure to increase. In trial one, the pressure was higher than in trial three because there were more reactants in trial one. In part two, my hypothesis was accepted because temperature and pressure have a directly proportionate relationship. References: Hart, M. H. The Evolution of the Atmosphere of the Earth. Icarus. 1978, 33, 23-39. Horvath, H Atmospheric Light Absorption- A Review. Atmos Environ. 1993, 27, 3, 293-317. Millero, F. J. Thermodynamics of the carbon dioxide system in the oceans. Geochim Cosmochim. Acta. 1995, 59, 4, 661-677.

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