The goal for this experiment was to see how much of both Sodium Bicarbonate and Acetic Acid it was going to take to fill you a sandwich bag without it exploding. We were going to need to figure out the volume of our bag and get the correct amount of each substance so when it fully reacts the gas formed can blow up the bag. The goal is to get it fully filled without it exploding or not filling up all the way. It’s like mixing baking soda and vinegar together it makes the same fizzy substance in a way along with a gas which most people use for volcanos. The airbag was invented in 1953 by an inventor in Newport , Pennsylvania. His name was John W. Hetrick and he came up this this idea to protect his family by using a lot of his old engineering
In this experiment, you have been asked by your teacher, to investigate the design of a small-scale airbag system they want to produce as a child safety device to put into baby strollers. Because of sodium azide’s toxicity (which is used in many vehicular airbags), it is suggested you use the reaction of NaHCO₃ (sodium bicarbonate or baking soda) with an aqueous solution of HCL (stomach acid) to produce CO₂ gas to test your engineering design. The reaction of hydrochloric acid and sodium bicarbonate is: HCL + NaHCO₃, one mole of CO₂ gas is produced. Regarding the other products, NaCl dissolves in the water to create a salt solution which occupies only a small portion of the volume inside the bag.
Throughout the course of the experiment, the weight of the beaker and liquid, the weight of the Alka-Seltzer tablet, the weight of the beaker with liquid plus the weight of the tablet, and the weight of the beaker with all of the contents after the bubbling ceased remained roughly constant and did not vary widely. However, a trend is able to be seen in Figure 1. It is clear that as the mL of vinegar used in each experiment run increased, the mass percent of NaHCO3 increased as well. During the construction of Figure 1, experiment runs four and six were deleted to create the expected graph which consists of a gradual increase and eventually leveling off into a plateau.
The moment an Alka-Seltzer tablet hits water, it begins to fizz. These tablets are over-the-counter antacids and pain relief medications that contain aspirin, sodium bicarbonate, and citric acid. The fizzing is a result of a reaction occurring where carbon dioxide (in the form of bubbles), water, and sodium acetate is formed. The fizzing and carbon dioxide bubbles are a result of the sodium bicarbonate splitting and reacting with the citric acid. In this experiment we are determining the percent by mass of sodium bicarbonate (NaHCO3) in Alka-Seltzer tablets and exploring the relationship between amounts of reactants and products.
The objective of the experiment was to observe different reactions with different chemicals. The experiments emphasized on the chemical changes occurring in acids and bases as well as color changes and bubble formations. The experiments allowed for a better understanding of the undergoing chemical changes in mixtures. Some mixtures instantly changed colors while others were transparent or foggy. Some mixtures produced thick color that created solids called precipitates. Mixtures KI + Pb(NO3)2 and NaOH + AgNO3 both produce noticeable precipitates after a while. It was interesting to see the different acidic and base reactions like the fuchsia color formation in NaOH + phenolphthalein.
After the amount of carbon dioxide lost was found, stoichiometry lets the loss of carbon dioxide to help find the amount of sodium bicarbonate reacted. Moreover, the mass of sodium bicarbonate and the mass of the original tablet help calculate the percent by mass of sodium bicarbonate. An observation made is that the changing amounts in each trial according to Table 1.1 show that, with changing amounts of starting material, the mass of carbon dioxide and the mass of sodium bicarbonate are inevitably affected. However, looking closely at Figure 1.1, the amounts of vinegar added increased in the experiment consequently making it the excess reactant to the sodium bicarbonate causing the graph in Figure 1.1 to level out. The tables should then show a steady increase in the percent by mass in the tablet and the amount of carbon dioxide
Stoichiometry with Kitchen Chemistry By: Meena Roberts Discussion Section: Wednesday at 8:30 Objective: The purpose of the lab was to see how much carbon dioxide was produced in reaction. Procedure: Measured mass of balloon, mass of NaHCO3 and container, mass of container after NaHCO3 was removed, and mass of NaHCO3 in balloon on digital scale in grams(g).
The outcome of the experiment was that the bag exploded when the chemicals mixed together and released off air pressure till the bag exploded. When doing this the experiment and watching the outcome had been surprising. The glycerine didn’t explode like the vinegar did in the first one because those chemicals never mixed. The tissue made the lab last alot longer. It didn’t matter if either the tissue was used to hold the baking soda in place, or the napkin. The results somewhat had matched up with the hypothesis of the bag exploding. On the other hand it was surprising that the lab to so
This invention is the ambulance. The invention of the ambulance began in 1859 when prototypes emerged in mass numbers. With ambulances, patients were now able to be transferred to other medical facilities more rapidly and efficiently. A man named Jonathan Letterman was appointed medical director of the Army of Potomac in 1862 and he immediately began to rework the structuring of the Ambulance Corps. He was able to combine the use of ambulances and he began to train enlisted men to be the Ambulance Core.
ABSTRACT Recently there has an increase in developing a new line of preserves that instantly inflates when a seal is ruptured and two chemicals are allowed to fuse together. Applicants need to formulate and test a formula that gives the volume of the life preserver that would produce the minimum weight of sodium bicarbonate. Also, that when mixed with an excess of 1.0M HCl, it would inflate the life preserver to the pressure of 1300 torr using the following equation, NaHCO3 + HCl CO2 + H2O + NaCl. The objective of this experiment was to find out what was the least amount of sodium bicarbonate needed to react with an excess of 1.0 M HCl to inflate the bag. We were able to determine that around 22 grams of sodium bicarbonate were needed to firmly inflate the bag without bursting.
Edward J. Claghorn put a patent on the “safety-belt” in 1885, and the safety-belt was for painters, firemen, etc. It was described as an object that was to be attached to a person so that they are secured to an object. Benjamin Foulois requested a seat belt for his military plane, but it wasn’t until World War II that the seat belt was used a lot. In 1955, Dr. Hunter Shelden came up with the idea of having seat belts in automobiles because of all the head injuries that were coming in.
2. Why is the mixture extracted with sodium bicarbonate? Give an equation and explain its relevance.
This experiment demonstrates the effects of sodium bicarbonate and citric acid in bath bombs on the pH of the water. The concept behind the experiment is to test if bath bombs are in fact safe to bathe in and what acids and bases do to pH. The amount of sodium bicarbonate and citric acid in the bath bombs vary throughout the experiment and act as the independent variable. The bath bombs in this experiment were dropped into a fish tank with three gallons of water in it. The pH was taken after the bath bomb had been in the water for eight minutes. The control group of bath bombs followed the original recipe without any modifications. These bath bombs resulted in the pH of the water being a six to a seven. The bath bombs with more sodium bicarbonate
Takata first entered into the automobile market in 1952 by producing seatbelts for automakers. In the 1980’s they began manufacturing airbags. As of 2014, they were one of leading producers of airbags, producing 20% of airbags used by automakers according to The New York Times. The rest of the market is split between two other suppliers. In the late 1990’s Takata did a redesign of their airbags to make them more compact and to reduce hazardous toxins. According to CNN, the company began using ammonium nitrate stored in a canister to inflate their airbags. Takata patent applications filed in 1999 states that there were problems with the gas which causes it to be unstable dependent on temperatures but they were working on a fix. They brought
The purpose of this experiment was to see if altering the ingredients of a bath bomb affected the effervescent when placed in water. When a bath bomb is submerged in water the ingredients caused it to fizz, releasing a scent and changing the color of the water. This bath bomb experiment requires two recipes, the first recipe which was labelled as “normal”, contained less cornstarch than the other recipe. In addition to the “normal” recipe, the other recipe was labelled “extra” because it contains more cornstarch. During this process, by adding or subtracting ingredients the eversences of the bath bomb changed. If more cornstarch is added to the recipe, the bath bomb will not fizz as much when placed in water. This is caused by the cornstarch,
have been found to cause injuries in so many accidents that the little good they