Developing A Model Airbag ATDP 2014
Developing a Model Airbag
Lucy Peng
Methods: To begin the experiment, my partner and I brainstormed several different airbag model designs: the first model containing a barrier of some sort to separate the NaHCO3 and the CH3COOH (Model 1) and the second model containing a “cup” or “pocket” taped to the wall of the plastic bag that would prevent the reactants form coming into contact (Model 2). We then measured arbitrary amounts of NaHCO3 using plastic weighing boats and an electronic scale.
We poured the NaHCO3 from the plastic weighing boats into their own plastic bags. Using the measurements of the NaHCO3 , we calculated the exact volumes of 6.0 M acetic acid needed to completely react with the amounts of NaHCO3 (see Calculations). The acetic acid was then measured out using 10 mL graduated cylinders and poured into their respective locations in the plastic bags. Once all of the reactants were placed into their correct positions, the bags were sealed and then rocked, shook, and flipped to simulate an automobile collision. Afterwards, we used a ruler measured the dimensions of each of the plastic bags in centimeters and recorded our observations in a lab notebook.
Results:
Table 1: Amount of Reactants; Comparison of Theoretical vs. Actual Volumes of CO2 Produced
Trial #
Mass of NaHCO3 (g)
Volume of 6M CH3COOH (mL)
Total mass of plastic bag and its contents
Theoretical Volume of the bag (L)
Actual Volume of the bag (L)
Percent Yield of CO2 1
0.802g
1.59 mL
4.20 g
214 cm3
169 cm3
79%
2
0.816 g
1.62 mL
3.38 g
219 cm3
389 cm3
178%
Trial 2 produced far more CO2 gas than Trial 1 and inflated the plastic bag the most despite having nearly the same reactant masses and volumes as Trial 1.
Calculations:
1. Determining the volume of 6 M CH3COOH (acetic acid) required to completely react with the mass of NaHCO3
NaHCO3 (s) + CH3COOH (aq) CO2 (g) + CH3COONa (aq) + H2O (l)
Given 0.8023 g of NaHCO3 (Trial 1)
Mole ratio 1 mol of NaHCO3 : 1 mol of CH3COOH
Molar
Lucy Peng
Methods: To begin the experiment, my partner and I brainstormed several different airbag model designs: the first model containing a barrier of some sort to separate the NaHCO3 and the CH3COOH (Model 1) and the second model containing a “cup” or “pocket” taped to the wall of the plastic bag that would prevent the reactants form coming into contact (Model 2). We then measured arbitrary amounts of NaHCO3 using plastic weighing boats and an electronic scale.
We poured the NaHCO3 from the plastic weighing boats into their own plastic bags. Using the measurements of the NaHCO3 , we calculated the exact volumes of 6.0 M acetic acid needed to completely react with the amounts of NaHCO3 (see Calculations). The acetic acid was then measured out using 10 mL graduated cylinders and poured into their respective locations in the plastic bags. Once all of the reactants were placed into their correct positions, the bags were sealed and then rocked, shook, and flipped to simulate an automobile collision. Afterwards, we used a ruler measured the dimensions of each of the plastic bags in centimeters and recorded our observations in a lab notebook.
Results:
Table 1: Amount of Reactants; Comparison of Theoretical vs. Actual Volumes of CO2 Produced
Trial #
Mass of NaHCO3 (g)
Volume of 6M CH3COOH (mL)
Total mass of plastic bag and its contents
Theoretical Volume of the bag (L)
Actual Volume of the bag (L)
Percent Yield of CO2 1
0.802g
1.59 mL
4.20 g
214 cm3
169 cm3
79%
2
0.816 g
1.62 mL
3.38 g
219 cm3
389 cm3
178%
Trial 2 produced far more CO2 gas than Trial 1 and inflated the plastic bag the most despite having nearly the same reactant masses and volumes as Trial 1.
Calculations:
1. Determining the volume of 6 M CH3COOH (acetic acid) required to completely react with the mass of NaHCO3
NaHCO3 (s) + CH3COOH (aq) CO2 (g) + CH3COONa (aq) + H2O (l)
Given 0.8023 g of NaHCO3 (Trial 1)
Mole ratio 1 mol of NaHCO3 : 1 mol of CH3COOH
Molar