Gas Laws Lab Report

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University of the People *

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1101

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Chemistry

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Dec 6, 2023

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Gas Laws Data Collection Following your detailed protocol based on the videos, perform all the experiments. Record your observations and take pictures of your key steps in the process. Your observations and images need to be incorporated in your data section and this section should be as detailed as possible as you will use this information to complete your discussion. Reaction of Baking Soda with Vinegar: 1. Prepare distilled white vinegar, baking soda, 100 mL graduated cylinder, digital scale, Erlenmeyer’s flask, balloon, strip of yarn, ruler, scissors, weighing boat, and plastic spoon.

2. Place weighing boat on scale and zero-out. Then measure EXACTLY 2.40 grams of baking soda. Adjust the amount with a plastic spoon if necessary. 3. Transfer the baking soda into the balloon. Pour 150 mL of distilled white vinegar into the Erlenmeyer’s flask. Then place the balloon onto the lip of the flask. *I am using an empty water bottle instead because I could not fit the balloon onto the flask that was provided in my kit. The lip was too wide. *I also ended up changing my balloon because there was a small hole found.

4. Dump the contents of the baking soda into the vinegar and watch the balloon inflate as the reaction is happening. Once over, carefully take off the balloon from the Erlenmeyer’s flask and knot it. 5. Wrap the yarn around the center of the balloon and trim off once the yarn meets the other end.

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6. Measure the length of the yarn in centimeters using the ruler. The circumference of the balloon is 40 cm. Scent Diffusion: 1. Prepare 2 balloons, a blueberry, lemon peels and 2 kitchen knives.

2. For the first balloon, place the blueberry inside and then squish into fine pieces. For the second balloon, place the lemon peel inside. Tear the lemon peel into fine pieces before placing inside the balloon. 3. Blow up both the balloons fully and knot them. Then place both balloons 2.5 ft away from your left and right side and with the kitchen knives, pop both balloons simultaneously and observe which scent diffused first. *My experiment did not turn out the way it should. As I was knotting the blueberry balloon, I accidentally punctured it with my fingernail. I could not redo this

experiment because I was only provided 3 balloons in my kit and one of them was already broken as I was doing the first experiment of this lab, so I only had 2 working balloons for this entire lab. Data Processing 1. Write the balanced chemical equation for the reaction observed in the first part of this experiment. NaHCO 3 (s) + HC 2 H 3 O 2 (aq)  NaC 2 H 3 O 2 (aq) + H 2 O(l) + CO 2 (g) 2. Assuming that all the baking soda from your balloon reacted, calculate how many moles of carbon dioxide gas would be formed. 2.40 g NaHCO 3 ∗ 1 mol NaHCO 3 84.01 g NaHCO 3 ∗ 1 molCO 2 1 mol NaHCO 3 = 0.0286 molCO 2 3. Assuming that all the acetic acid (assume 5% by mass with a density of 1.006 g/ml) from your Erlenmeyer flask reacted, calculate how many moles of carbon dioxide gas would be formed. 150 mL HC 2 H 3 O 2 ∗ 1.006 g HC 2 H 3 O 2 1 mL HC 2 H 3 O 2 = 150.9 g HC 2 H 3 O 2 ( whole ) 5% HC 2 H 3 O 2 ∗ 150.9 g HC 2 H 3 O 2 ( whole ) 100% HC 2 H 3 O 2 = 7.545 g HC 2 H 3 O 2 ( part ) 7.545 g HC 2 H 3 O 2 ∗ 1 mol HC 2 H 3 O 2 60.05 g HC 2 H 3 O 2 ∗ 1 molCO 2 1 mol HC 2 H 3 O 2 = 0.1256 molCO 2 4. Using your calculations, identify the limiting reactant of your reaction and determine the maximum amount (in moles) of carbon dioxide that could be produced. The limiting reactant of this reaction is clearly the baking soda because it produced the least amount of carbon dioxide. However, the maximum amount of carbon dioxide that can be produced is 0.1256 moles.

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5. Using your calculated number of moles of carbon dioxide from Question 4, the atmospheric pressure, the vapor pressure of water at your room temperature, and your room temperature value, calculate the expected volume of the balloon. Given: 0.0286 mol CO 2 limiting reactant 23°C (296.15 K) 1 atm – 21.1 = 20.1 atm V = 0.0286 molCO 2 ∗ 8.3144598 R ∗ 296.15 K 20.1 atm = 3.504 L 6. Using your measurement for the circumference of the balloon, calculate the volume of the gas in the balloon. r = 40 cm 2 pi = 6.366 cm V = 4 3 ∗ π ∗ 6.366 3 = 1081 mL = 1.081 L 7. Using the expected and the measured volumes of the carbon dioxide, calculate the percent yield of the experiment. 1.081 L ( actual ) 3.504 L ( expected ) ∗ 100 = 30.85% 8. Calculate the expected volume for 1 mole of an ideal gas under atmospheric pressure and your room temperature conditions. V 1 mol = 0.0831 R ∗ 296.15 K 1 atm V = 24.61 L / mol 9. Using your measured gas volume and calculated moles from Question 4, calculate the molar volume of your collected carbon dioxide gas. 1.081 L ( actual ) 0.0286 molCO 2 = 37.8 L / mol

10.Considering the value calculated in Question 8 the correct value for the molar volume under your reaction conditions, calculate the error for the molar volume in your experiment. (Hint: the calculated value from Question 9 is your experimental molar volume.) 37.8 L mol ( actual ) − 24.61 L mol ( expected ) 24.61 L mol ( expected ) ∗ 100 = 53.60% 11.Identify the compound responsible for the scent of the two materials you selected for the scent diffusion experiment and draw their structural formula. Ethyl Octanoate, C 10 H 20 O 2 , is responsible for the blueberry scent. Beta-Cyclocitral, C 10 H 13 O, is responsible for the lemon scent. 12.Using the formula for the root mean-square velocity of gases, your room temperature values and the molar masses of the two compounds from Question 11, identify which scent should you smell first if the balloons were popped at the same time. If the balloons were popped at the same time, we should smell the blueberry one first because it has a stronger scent and more moisture than the lemon peel. 13. Fill in the following table using the observations and data from your experiments. Assumptions made Testing the assumption If assumptions are wrong ...

All the baking soda is consumed in the reaction. Shake the Erlenmeyer’s flask a little to further combine the baking soda with the vinegar. The reaction is still happening because the vinegar has yet to fully consume the baking soda. The gas production from the baking soda and vinegar is not inflating the balloon. Hold the lip of the balloon onto the lip of the flask so that no gas escapes out of the balloon as the reaction is happening. The balloon is not inflating due to either having holes in it or not grasping it tightly onto the flask. Both the blueberry and lemon peel diffused scent at the same time. Pop both balloons at the same time and observe which balloon first diffused scent. The blueberry was the first one to diffuse since it has a stronger scent than the lemon peel. Crushing the scented fruits or veggies does not make a difference in scent diffusion. Perform the experiment again, this time leaving the fruits intact inside the balloon. There is little to no scent coming from the balloons after popping. Student 1 Data:  Percent Yield: 27.2%  Actual Molar Volume: 2.67 L/mol Student 2 Data:  Percent Yield: 61.5%  Actual Molar Volume: 15.3 L/mol Student 3 Data:  Percent Yield: 23.75%  Actual Molar Volume: 40.6 L/mol Discussion Write a minimum one page (12 font, single spaced) discussion on the experiment conducted this week. Address at least one question in each category as fully as possible integrating the collected data, providing explanations for the observed trends and evaluating whether your original assumptions about the experiment were validated

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by the results. The assignment will be graded on completeness, clarity of the explanations and the meaningful integration of the collected and calculated data. Correct grammar and appropriate format for the chemical formulae and chemical reactions is expected. Ideal gases are hypothesized gases in which the molecules take up minimal space and do not have any interactions, hence obeying the gas laws perfectly. A real gas will behave as an ideal gas if they are at lower pressure and higher temperatures. By enlarging the volume around every particle, low pressure reduces the influence of the real particles' fixed size. High temperatures provide the particles with sufficient kinetic energy to escape the actual attractions that keep them from adhering together. In general, real gases behave as ideal gases from freezing or condensation and if they are distant from the phase boundary. The balanced chemical equation in this first part of the experiment where the baking soda reacts with the distilled white vinegar is: NaHCO 3 (s) + HC 2 H 3 O 2 (aq)  NaC 2 H 3 O 2 (aq) + H 2 O(l) + CO 2 (g). In the microscopic scale, this means the baking soda or sodium bicarbonate dissolves and reacts with the vinegar or acetic acid where the molecules would rearrange to produce sodium acetate, water, and carbon dioxide gas. However, on the macroscopic scale, the human eye would only see the mixture temporarily foam up and produce carbon dioxide gases much like pouring out soda in a cup. The gas inside a can of soda is the same gas found in the baking soda and vinegar reaction. Comparing my percent yield values to my group’s percent yield values, we were all off by a significant amount. My percent yield was 30.85%, student 1’s was 27.2%, student 2’s was 61.5%, and student 3’s was 23.75%. Student 2’s data was the outlier here because his was significantly higher than the rest of us at the 20% to 30% range. Therefore, our data would neither be accurate nor precise. A data is only accurate if it is off by 1% and a data is only precise if it is off at the decimal amount. We can assume that our CO 2 would be suitable for this experiment because we used the balloon to capture and trap in the gas as the reaction with the baking soda and vinegar was happening. CO 2 is only soluble in water if the pressure is kept. Once the pressure is gone, all the CO 2 will get released into the air. If this assumption were to be invalid, there would be little to no gas formation inside the balloon and the balloon would not inflate. The purpose of this experiment was to observe the biproducts produced when baking soda and vinegar gets reacted together and to observe in the scent diffusion experiment which balloon diffused the scent the soonest. One thing that would be changed in the diffusion experiment to improve it would be to use a regular sandwich bag instead of a balloon and then cut open both bags at the same time because I ended

up accidentally popping one of the balloons as I was knotting it. By performing this experiment, I learned that CO 2 is found almost everywhere in the air and certain carbonated drinks such as sodas and sparkling water.