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Airbag Detonation Simulation

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Introduction

Lekha Ravichandran Class #5/6 11/9/08 Airbag Detonation Simulation: METHOD: 1. Measure the volume of the zip-loc bag by filling it completely up with water (make sure there are no air bubbles!) and pouring it into a large 500mL graduated cylinder. 2. Record the volume 3. Record the given temperature and pressure that the teacher puts on the board in the data table 4. Use the ideal gas law to find the moles of Carbon Dioxide present. (PV=nRT - you are trying to find "n") 5. Using the balanced reaction of baking soda and hydrochloric acid (NaHCO3 + HCl --> H20 + C02 + NaCl), it is evident that the mole ratio between carbon dioxide and hydrochloric acid would be one-to-one. 6. Using the moles of hydrochloric acid needed, figure out the volume needed of HCl from its 0.50 M concentration. 7. Subtract the volume of HCl from the original volume of the zip-loc that was measured in the beginning (this is because the HCl will occupy the space of the bag once it is added). ...read more.

Middle

= n (0.08206 mol*K/L*atm) 293.4 K 0.0497 mol CO2 = n VOLUME OF HYDROCHLORIC ACID: NaHCO3 + HCl --> H20 + C02 + NaCl 0.0497 mol C02 --> 0.0497 mol HCl (b/c of 1:1 mole ratio) WORK: AMOUNT OF BAKING SODA: 1.2 L - 0.0094 L = 1.1006 L PV=nRT P= 0.997 atm V= 1.1006 L T= 293.4 K R= 0.08206 mol*K/L*atm WORK: 0.997 atm (1.1006 L) = n (0.08206 mol*K/L*atm) 293.4 K 0.0456 mol NaHCO3 = n 0.0456 mol NaHCO3 (84.01 g NaHCO3 / 1 mol NaHCO3) = 3.83 g NaHCO3 CONCLUSION: This experiment was conducted in order observe the reaction between baking soda and hydrochloric acid. The products I got from these two reactants were carbon dioxide, water, and sodium chloride. The gas formed by this reaction is what made the bag inflate once I mixed the reactants together. In order to figure out how much of the reactants to add, I used the ideal gas law with the information given to me in the background information to calculate the amounts. My first trial, using 99.4 mL HCl and 3.83 g NaHCO3, had insufficient reactants because not enough gas occupied the bag in order to fill the bag to plumpness. ...read more.

Conclusion

This would change the results I calculated when using the ideal gas law. Since the actual yield of gas was most likely to be lower than we assume for it to be, as with any products that are made in a chemical reaction, I might have had to add more reactants than what it said in my calculations - which means that I would have to add even more than what I used in my second trail. Moreover, all the reactants did not completely mix since some baking soda got caught in the corners of the bag, which could have led to less gas being able to form. The most major source of error was probably trying to avoid mixing the baking soda and hydrochloric acid since that would have allowed some gas to escape from the bag before closing it. As it is evident, my bag underinflated because not enough gas was produced to bring it to "plumpness". In the future, as I aforementioned, adding more reactants would solve this problem and also calculating the percent yield of carbon dioxide in the reaction since my results indicates that it will not be a 100% yield. ...read more.

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