Sit at least 25 centimetres from the steering wheel. This way, if the airbag deploys, it will cushion rather than injure you. Do not sleep resting against a window — when the side curtain airbag deploys it may injure you. Replace an airbag right away if it has deployed or is broken. Children and airbags Never place an infant or child near an active airbag.
These manuals will tell you where you can safely place your child and their seat. Was this page helpful? How can we improve this page? How did this page help you? Leave this field blank. This allows for bumper bashing and minor bumps - like parking your car in the garage and hitting your wall accidentally - to occur without the deployment of airbags. High speed video and film were used to record the deployments, and a pressure transducer measured the airbag's internal pressure.
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This bar graph shows that there is a significantly higher reduction in moderate to serious head injuries for people using airbags and seat belts together than for people using only seat belts. Timing is crucial in the airbag's ability to save lives in a head-on collision. An airbag must be able to deploy in a matter of milliseconds from the initial collision impact. It must also be prevented from deploying when there is no collision. Hence, the first component of the airbag system is a sensor that can detect head-on collisions and immediately trigger the airbag's deployment.
One of the simplest designs employed for the crash sensor is a steel ball that slides inside a smooth bore. The ball is held in place by a permanent magnet or by a stiff spring, which inhibit the ball's motion when the car drives over bumps or potholes. However, when the car decelerates very quickly, as in a head-on crash, the ball suddenly moves forward and turns on an electrical circuit, initiating the process of inflating the airbag. Once the electrical circuit has been turned on by the sensor, a pellet of sodium azide NaN 3 is ignited.
A rapid reaction occurs, generating nitrogen gas N 2. This gas fills a nylon or polyamide bag at a velocity of to miles per hour. This process, from the initial impact of the crash to full inflation of the airbags, takes only about 40 milliseconds Movie 1. Ideally, the body of the driver or passenger should not hit the airbag while it is still inflating.
In order for the airbag to cushion the head and torso with air for maximum protection, the airbag must begin to deflate i. Otherwise, the high internal pressure of the airbag would create a surface as hard as stone-- not the protective cushion you would want to crash into!
Please click on the pink button below to view a QuickTime movie showing the inflation of dual airbags when a head-on collision occurs. Click the blue button below to download QuickTime 4. When the car undergoes a head-on collision, a series of three chemical reactions inside the gas generator produce gas N 2 to fill the airbag and convert NaN 3 , which is highly toxic The maximum concentration of NaN 3 allowed in the workplace is 0.
The signal from the deceleration sensor ignites the gas-generator mixture by an electrical impulse, creating the high-temperature condition necessary for NaN 3 to decompose. The nitrogen gas that is generated then fills the airbag. The purpose of the KNO 3 and SiO 2 is to remove the sodium metal which is highly reactive and potentially explosive, as you recall from the Periodic Properties Experiment by converting it to a harmless material.
The N 2 generated in this second reaction also fills the airbag, and the metal oxides react with silicon dioxide SiO 2 in a final reaction to produce silicate glass, which is harmless and stable. First-period metal oxides, such as Na 2 O and K 2 O, are highly reactive, so it would be unsafe to allow them to be the end product of the airbag detonation.
This table summarizes the species involved in the chemical reactions in the gas generator of an airbag. Nitrogen is an inert gas whose behavior can be approximated as an ideal gas at the temperature and pressure of the inflating airbag. Thus, the ideal-gas law provides a good approximation of the relationship between the pressure and volume of the airbag, and the amount of N 2 it contains.
A certain pressure is required to fill the airbag within milliseconds. Once this pressure has been determined, the ideal-gas law can be used to calculate the amount of N 2 that must be generated to fill the airbag to this pressure. The amount of NaN 3 in the gas generator is then carefully chosen to generate this exact amount of N 2 gas. An estimate for the pressure required to fill the airbag in milliseconds can be obtained by simple mechanical analysis.
Assume the front face of the airbag begins at rest i. Note: In the calculation below, we are assuming that the airbag is supported in the back i. Note: The pressure calculated is gauge pressure.
The amount of gas needed to fill the airbag at this pressure is then computed by the ideal-gas law see Questions below. Note: the pressure used in the ideal gas equation is absolute pressure. When N 2 generation stops, gas molecules escape the bag through vents. T he pressure inside the bag decreases and the bag deflates slightly to create a soft cushion.
By 2 seconds after the initial impact, the pressure inside the bag has reached atmospheric pressure. Thus far, we have only considered the macroscopic properties i. Now we turn to a theoretical model to explain these macroscopic properties in terms of the microscopic behavior of gas molecules.
The kinetic theory of gases assumes that gases are ideal i. In a microscopic view, the pressure exerted on the walls of the container is the result of molecules colliding with the walls, and hence exerting force on the walls Figure 3. When many molecules hit the wall, a large force is distributed over the surface of the wall. This aggregate force, divided by the surface area, gives the pressure. This is a schematic diagram showing gas molecules purple in a container.
The molecules are constantly moving in random directions. When a molecule hits the container wall green , it exerts a tiny force on the wall. The sum of these tiny forces, divided by the interior surface area of the container, is the pressure. An important relationship derived from the kinetic theory of gases shows that the average kinetic energy of the gas molecules depends only on the temperature. Thus, we can view temperature as a measure of the random motion of the particles, defined by the molecular speeds.
We see from the kinetic theory of gases that temperature is related to the average speed of the molecules. This implies that there must be a range distribution of speeds for the system. In fact, there is a typical distribution of molecular speeds for molecules of a given molecular weight at a given temperature, known as the Maxwell-Boltzmann distribution Figure 4.
This distribution was first predicted using the kinetic theory of gases, and was then verified experimentally using a time-of-flight spectrometer.
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