6-2 Engineering a Better Air Bag Lab Report Dr Z Edits

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Jan 9, 2024

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Engineering a Better Airbag Kristen Brown 12/4/2023 Data Use 0.0821 L ∗ atm mol ∗ K for R. Data Table 1: Model Air Bag Activity Data and Calculations Volume of 6 × 9 inch bag 1.20 L Room temperature (in K) 25 °C + 273.15 = 298.15 K Room pressure (in atm) 1 atm Moles of CO 2 required to inflate bag at room temperature and pressure. Show work, including all units, in the space provided. N = 1 atm * 1.2 L / (0.0821L - atm/mole * K) * 298.15K = 1.2/24.478115 = 0.05 mol of CO 2 Balanced equation for the reaction of NaHCO 3 and CH 3 COOH 1. NaHCO 3 (s) + CH 3 COOH(aq) ➝ CH 3 COONa(aq) + H 2 O(l) + CO 2 (g) 3. H 2 O(l) + CO 2 (g) + CH 3 COONa(aq) → NaHCO 3 (aq) + CH 3 COOH(aq) Mass of NaHCO 3 needed for the reaction. Show work, including all units, in the space provided. 4.2g NaHCO 3 0.05mol * 84.0g = 4.2g Volume of vinegar required (0.833 M acetic acid) Show work, including all units, in the space provided. (0.05molCO 2 * CH 3 COOH/CO 2 ) / 0.833mol (0.05molCO 2 )/0.833mol/L * 1000 = 60.02mL ****If you did not use molar ratios in the calculations for Mass NaHCO 3 and Volume of Vinegar you are completing the calculation incorrectly.****

Data Table 2: Model Air Bag Trial # NaHCO 3 (grams) Vinegar (mL) Observations 1 4.2g 60.2 Foamed up slowly; bag was only filled about halfway with gas 2 4.5g 65.2 Quicker reaction time; increase of foam and bag filled up more than last trial but the bag wasn’t taught with gas 3 4.7g 75.2 Very quick reaction; bag filled quickly with gas and was almost taught to the touch. Would provide adequate cushion in the incident of a car accident Data Table 3: 80-L Driver-Side Air Bag Activity Data and Calculations Moles of CO 2 required to inflate 80L bag at room temperature and pressure. Show work, including all units, in the space provided. (1 atm * 80L) / (298.15K * 0.0821 L * atm/mol*k) = 80/24.478115 = 3.26822551 = 3.3 moles of CO 2 Balanced equation for the reaction of NaHCO 3 and CH 3 COOH NaHCO 3 + CH 3 COOH → CH 3 COONa + H 2 O + CO 2 Mass of NaHCO 3 needed for the reaction. Show work, including all units, in the space provided. 1:1 ratio Mass = Moles * Molar mass 84.0 g/mol * 3.3moles CO 2 = 277.2g NaHCO 3 Volume of vinegar required (0.833 M acetic acid) Show work, including all units, in the space provided. 1:1 ratio Volume = Moles / Molarity Volume = 3.3 moles / 0.833 M = 3.96 L of vinegar ****If you did not use molar ratios in the calculations for Mass NaHCO 3 and Volume of Vinegar you are completing the calculation incorrectly.**** Data Table 4: 160-L Front Passenger-Side Air Bag Activity Data and Calculations Moles of CO 2 required to inflate 160 L bag at room temperature and pressure. Show work, including all units, in the space provided. (1 atm* 160L)/ (298.15K * 0.0821L * atm/mol*k) = 160/24.478115 = 6.5 moles of Co 2 ©2016 2 Carolina Biological Supply Company

Balanced equation for the reaction of NaHCO 3 and CH 3 COOH NaHCO 3 + CH 3 COOH → CH 3 COONa + H 2 O + CO 2 Mass of NaHCO 3 needed for the reaction. Show work, including all units, in the space provided. 1:1 ratio Mass = Moles * Molar mass Mass = 6.5 moles CO 2 × 84.0 g/mol = 546 g NaHCO 3 Volume of vinegar required (0.833 M acetic acid) Show work, including all units, in the space provided. 1:1 ratio Volume = Moles / Molarity Volume = 6.5 moles / 0.833 M = 7.8 L of vinegar ****If you did not use molar ratios in the calculations for Mass NaHCO 3 and Volume of Vinegar you are completing the calculation incorrectly.**** Question 1: Based upon the observed performance of the air bag models and the amounts of sodium bicarbonate and acetic acid (vinegar) needed for an automotive air bag of 80 or 160 L, are these reactants a good substitute for sodium azide? One additional note regarding sodium azide: the rate of inflation after a triggering impact is 40 milliseconds (0.04 s). While the reaction between sodium bicarbonate and acetic acid can produce gas and could theoretically be used to inflate an airbag, it wouldn’t be a practical or effective substitute for sodium azide in a real-world application. This is due to the slower reaction speed, reaction conditions (having to use an aqueous solution could pose challenges in the design/durability of the system), the amount of gas produced (would require larger amounts of reactants to inflate the same volume, which would increase the size and weight of the airbag system), and safety (concerns of accidental deployment and leakage of reactants). ©2016 2 Carolina Biological Supply Company

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