K2O: Reacts with the third compound of the original airbag mixture, silicon dioxide, to form alkaline silicate that is harmlessly discarded in a deployed airbag. Stoichiomety is very important to the PROPER function of airbags. With out the careful calculations and measurements airbags a life saving device would be life threatening.
Why is stoichiometry important for airbags?
A typical air bag contains approximately 130 g of NaN3 that can produce 67 L of N2 gas when NaN3 decomposes. If an insufficient amount of nitrogen were produced, the air bag would under inflate and not provide adequate protection. Clearly, the stoichiometry of the reaction is very important.
What is the chemistry behind an airbag?
The chemical at the heart of the air bag reaction is called sodium azide, or NaN3. CRASHES trip sensors in cars that send an electric signal to an ignitor. The heat generated causes sodium azide to decompose into sodium metal and nitrogen gas, which inflates the car's air bags.
What is the importance of stoichiometry in chemistry?
Why Stoichiometry Is Important. You can't understand chemistry without grasping the basics of stoichiometry because it helps you predict how much of a reactant participates in a chemical reaction, how much product you'll get, and how much reactant might be left over.
What is one of the most important aspect of airbags?
Airbags are proven safety devices Airbags provide particularly effective protection against severe or deadly impacts to the head or chest. In the event of a collision, airbags inflate to prevent drivers and passengers from hitting their heads against the steering wheel, dashboard, side windows or door frames.
How fast does the chemical reaction of the airbag take?
The heat from the ignition causes nitrogen gas to generate, fully inflating the airbag in . 03 seconds.
How does Boyle's law apply to airbags?
Gas laws related to airbags Boyle's Law- When the airbag expands, the pressure decreases as the volume increases at a constant temperature.
What is stoichiometry in chemistry definition?
Definition of stoichiometry 1 : a branch of chemistry that deals with the application of the laws of definite proportions and of the conservation of mass and energy to chemical activity. 2a : the quantitative relationship between constituents in a chemical substance.
How can you apply the concept of stoichiometry in your life?
Let's take a look at few examples of how stoichiometry is being employed in practical life.Airbags Design.Rocket Propulsion.Lithium Hydroxide Scrubber.Pharmaceutical Industry.Role in Fast-moving consumer goods (FMCGs)Green Chemistry.Ecological Stoichiometry.
What is stoichiometry explain with example?
One molecule of methane reacts with two molecules of oxygen gas to yield one molecule of carbon dioxide and two molecules of water. Stoichiometry measures quantitative relationships, and is used to determine the amount of products/reactants that are produced/needed in a given reaction.
How do you verify the satisfactory function of the airbag?
There is an airbag indicator light on the dashboard. To see it, simply turn the ignition key to the first position, and pause there. This is the indicator light test position. You should see all the indicator lights turn on, including the airbag light.
What are the 3 main parts of an airbag?
The airbag module contains both an inflator unit and the lightweight fabric airbag. The airbag system consists of three basic parts: (1) An airbag module, (2) crash sensors, and (3) a diagnostic unit. Some systems may also have an on/off switch, which allows the airbag to be deactivated.
How do airbags work physics?
The bag itself has tiny holes that begin releasing the gas as soon as it's filled. The goal is for the bag to be deflating by time your head hits it. That way it absorbs the impact, rather than your head bouncing back off the fully inflated airbag and causing you the sort of whiplash that could break your neck.
How do airbags work physics?
The bag itself has tiny holes that begin releasing the gas as soon as it's filled. The goal is for the bag to be deflating by time your head hits it. That way it absorbs the impact, rather than your head bouncing back off the fully inflated airbag and causing you the sort of whiplash that could break your neck.
Do airbags release chemicals?
Airbags cause no chemical injuries. The sodium azide they contain is used up when they deploy, and the gas produced, nitrogen, is not harmful (The air we breathe is 78% nitrogen). The dust released from air bags may have some sodium hydroxide in it. This may be mildly irritating.
Why is potassium nitrate also in airbags?
The first automotive airbags developed in the 1970s employed a solid propellant. These airbag inflation systems reacted sodium azide (NaN3) with potassium nitrate (KNO3) in order to produce nitrogen gas. Hot blasts of nitrogen gas inflated the airbag.
Can you get a chemical burn from an airbag?
Chemical burns — highly alkaline gasses and chemicals emitted from airbags often cause burns. These substances can penetrate the skin and cause deep tissue injuries in some cases. Thermal burns — exposure to high temperature gas from the explosion of chemicals that affect the hands, arms and chest.
What gas is produced when a bag is squished?
The chemicals will begin to react and bubble; the gas that is produced is carbon dioxide (CO 2 ). The bag should begin to inflate. When the bubbling stops, further mix the acetic acid and sodium bicarbonate by squishing and/or shaking the bag to make sure the reaction proceeds as far as possible.
How have airbags saved lives?
They have undoubtedly saved lives, especially in accidents when the driver or passengers neglected to use seatbelts. Airbags have saved many lives, but only when they deploy properly. Recently, however, millions of cars have been recalled due to defective airbags that were not properly designed or manufactured.
Can you leave sodium bicarbonate in a bag?
There also should not be any sodium bicarbonate or acetic acid left in the bag. Before starting, look at the attached data table in which you will record the amount of acid, the amount of sodium bicarbonate, a description of how the bag inflated, and whether there was acetic acid or sodium bicarbonate left over.
What chemical reaction is used to decompose an airbag?
This requirement is satisfied in many automotive airbag systems through use of explosive chemical reactions, one common choice being the decomposition of sodium azide, NaN 3. When sensors in the vehicle detect a collision, an electrical current is passed through a carefully measured amount of NaN 3 to initiate its decomposition:
Why do airbags deploy?
Airbags deploy upon impact to minimize serious injuries to passengers. Image credit: Jon Seidman.
Learning Objectives
Explain the concept of stoichiometry as it pertains to chemical reactions
Example 4.8
How many moles of I 2 are required to react with 0.429 mol of Al according to the following equation (see Figure 4.9 )?
Example 4.9
How many carbon dioxide molecules are produced when 0.75 mol of propane is combusted according to this equation?
Answer
These examples illustrate the ease with which the amounts of substances involved in a chemical reaction of known stoichiometry may be related. Directly measuring numbers of atoms and molecules is, however, not an easy task, and the practical application of stoichiometry requires that we use the more readily measured property of mass.
Example 4.10
What mass of sodium hydroxide, NaOH, would be required to produce 16 g of the antacid milk of magnesia [magnesium hydroxide, Mg (OH) 2] by the following reaction?
Example 4.11
What mass of oxygen gas, O 2, from the air is consumed in the combustion of 702 g of octane, C 8 H 18, one of the principal components of gasoline?
Answer
These examples illustrate just a few instances of reaction stoichiometry calculations. Numerous variations on the beginning and ending computational steps are possible depending upon what particular quantities are provided and sought (volumes, solution concentrations, and so forth).
Why do airbags work?
An airbag is designed to release some of the gas just after it deploys to help cushion the impact against the body. Hitting a fully inflated, unyielding airbag could be catastrophic. So before widely promoting this protective device, the safety of the contents had to be ascertained. In the 1970s Mercedes settled this issue by putting a cage full of canaries in a car and deploying an airbag. Canaries are extremely sensitive to minute traces of toxic gases but the birds survived the experiment with no casualties. By the late 1980s airbags had become a common feature in automobiles and have since saved thousands of lives.
What chemical is used to inflate airbags?
The answer would be found in a fascinating chemical called sodium azide, NaN3. When this substance is ignited by a spark it releases nitrogen gas which can instantly inflate an airbag. The problem, however, is that the reaction also forms sodium metal which reacts with moisture to generate sodium hydroxide, a highly corrosive substance. A burst airbag could wreak havoc. Chemical ingenuity, however, came to the fore. If potassium nitrate and silicon dioxide were also included with the sodium azide, the only products that would form in addition to nitrogen would be potassium silicate and sodium silicate. Both of these are inert, harmless substances.
What would happen if an airbag burst?
A burst airbag could wreak havoc. Chemical ingenuity, however, came to the fore. If potassium nitrate and silicon dioxide were also included with the sodium azide, the only products that would form in addition to nitrogen would be potassium silicate and sodium silicate. Both of these are inert, harmless substances.
How fast can an airbag go?
The most serious concern, however, is damage that can be done by an airbag as it rockets out at an astounding speed of up to 330 km per hour. A blow to the head by the rapidly inflating bag can be lethal.
When did airbags become common?
By the late 1980s airbags had become a common feature in automobiles and have since saved thousands of lives. But, like with any other scientific advance, there is a “but.”. Airbags are not problem-free. While the chemistry involved in curbing sodium hydroxide production is clever, it is not foolproof.
When was the first airbag invented?
Soon Hetrick came up with a prototype and in 1952 was granted the first patent for what would become the predecessor to the airbag. The original idea of using compressed air turned out to be not workable because the air cylinder itself represented a risk.
Who invented airbags?
The Fascinating Chemistry of Airbags. The original idea for airbags seems to have been born in the fertile mind of none other than Leonardo de Vinci. "Baghe di vento,” or “bags of air” he called his invention, which was certainly not designed for cars. It was designed for flying men. Or at least, for men who were attempting to fly.
Introduction
Objective
- Working in a group you will investigate the underlying chemistry of airbags and design, build and test your own “airbag” to see if it can protect a “passenger.” Part 1 This lab begins with an internet exploration of how car air bags work. Your report should answer the following questions and indicate references used. To get started, here are a few references: 1. HowStuffWorks: How Air …
Pre-Lab Questions
- What is the intended purpose of an air bag?
- How does an air bag deploy? Describe the process.
- What is the chemistry behind an air bag? Write the balanced main chemical reaction and secondary reactions. Note: Not all air bags have the same secondary reaction.
- What gas fills the air bag? Why was this gas chosen to use in an air bag?
Background
- In the second part of the project you are to design and build your own airbag utilizing sodium bicarbonate (baking soda) and acetic acid (vinegar). NaHCO3(s) + CH3COOH(aq)→ CO2(g) + CH3COONa(aq) + H2O(l) Your task is to find the correct amounts of sodium bicarbonate and acetic acid to use to create the right amount of gas (carbon dioxide) to fill the bag. If done corre…
Hypothesis
- Which bag do you predict will produce the greatest amount of CO2? Circle your prediction. bag #1 - 25 mL of vinegar + 0.5 g of sodium bicarbonate bag #2 - 25 mL of vinegar + 1.0 g of sodium bicarbonate bag #3 - 25 mL of vinegar + 1.5 g of sodium bicarbonate bag #4 - 25 mL of vinegar + 2.0 g of sodium bicarbonate bag #5 - 25 mL of vinegar + 2.5 g of sodium bicarbonate bag #6 - 2…
Procedure
- Mass 0.5 grams of sodium bicarbonate (NaHCO3) and record the exact mass in the data table. Carefully pour it from the weighing boat into a bag. Flatten the bag to remove any air.
- Add 25 mL of acetic acid (vinegar) to the bag and seal the bag as quickly as possible. Start the timer. The bag should begin to inflate. The chemicals will begin to react and bubble; the gas that i...
- Mass 0.5 grams of sodium bicarbonate (NaHCO3) and record the exact mass in the data table. Carefully pour it from the weighing boat into a bag. Flatten the bag to remove any air.
- Add 25 mL of acetic acid (vinegar) to the bag and seal the bag as quickly as possible. Start the timer. The bag should begin to inflate. The chemicals will begin to react and bubble; the gas that i...
- When the bubbling stops, further mix the acetic acid and sodium bicarbonate by squishing and/or shaking the bag to make sure the reaction proceeds as far as possible. When no more bubbles are produ...
- The test how inflated the bag is by pinching it. Write a description and rank the fullness of the bag in the data table. Also, does the bag feel warm or cold? Make a note of that.
Analysis
- Write the balancedchemical equation. What is the mole ratio of acetic acid and sodium bicarbonate? What is the molar mass of acetic acid? What is the molar mass of sodium bicarbonate?
- Assuming acetic acid is 5% and has a density of 1g/ml, calculate how many moles of acetic acid in bags 1-6. Enter the values in the table. Mass of acetic acid: 25ml x (1g/1ml) x (5%) = 1…
- Write the balancedchemical equation. What is the mole ratio of acetic acid and sodium bicarbonate? What is the molar mass of acetic acid? What is the molar mass of sodium bicarbonate?
- Assuming acetic acid is 5% and has a density of 1g/ml, calculate how many moles of acetic acid in bags 1-6. Enter the values in the table. Mass of acetic acid: 25ml x (1g/1ml) x (5%) = 1.25g
- Calculate how many moles of sodium bicarbonate there are in bags 1-6. Enter the values in the table.
- Calculate how many moles of CO2formed in bags 1-6. Enter the values in the table.