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What is the point of silicon dioxide? 8. Why are careful stoichiometric calculations important for air bags and safety?

What is the point of silicon dioxide? 8. Why are careful stoichiometric calculations important for air bags and safety?

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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7.What is the point of silicon dioxide?
8. Why are careful stoichiometric calculations important for air bags and safety?
Chemistry in Action Air Bags and Stoichiometry Air bags are part of the mandatory safety systems in passenger vehicles currently sold in the United States. An air bag inflates upon collision and prevents the driver or passenger from hitting the steering wheel, dash- board, or windshield. An air bag also absorbs some of the force resulting from the collision by immediately deflating through vents when the dri- ver or passenger hits the air bag Air bags are amazing devices. They must inflate within 0.04 seconds of a collision. Because a collision cannot not provide adequate protection. Clearly, the stoichiometry of the reaction is very important. The safety of the chemical products produced in air bags is also an impor- reactive to be considered safe. A third ingredient, silicon dioxide, SiO2, the main ingredient in sand, reacts with the sodium oxide and potassium oxide to form a safe, stable silicate glass. As a result, all of the harmful products generated during the air bag inflation are converted into safe substances. tant consideration. Sodium azide is highly toxic, but it is entirely con- sumed in the decomposition reaction. The sodium that is produced by the sodium azide decomposition can react explosively with water to produce sodium hydroxide and hydrogen. Potassium nitrate, KNO, is mixed with the sodium azide because KNO3 can react with the sodium metal to pro- duce safer compounds, as shown in the following unbalanced equation: However, the reaction of the potassi- um nitrate with the sodium metal also produces nitrogen gas, which will increase the volume of gas inside the air bag. Careful stoichiometric calcula- tions are needed to choose the correct amount of reactants to yield the total volume of nitrogen required for the air bag to function properly. be predicted, the inflation system must be ready to activate at any time during the life of the vehicle. The rapid chemical decomposition of solid sodi- um azide, NaN, allows the air bag to inflate fast at any time. The decompo- sition reaction is initiated in a car by a small ignition induced by a collision sensing mechanism. The nitrogen gas produced during the reaction inflates the air bag. Although NaN, is stable at room temperature, it decomposes into solid sodium and nitrogen gas at tem- peratures above 300°C by the reac- tion shown beloW. KNO,(s) + Na(s)→ Question 1. Balance the equation for the reaction of potassium nitrate K,0(s) + Na,0(s) + N2(g) Another chemical reaction is still required because the potassium oxide, K,0, and sodium oxide, Na,O, are too and sodium. V An air bag inflates with nitrogen in 0.04 seconds. 2NAN3(s) → 2Na(s) + 3N,(g) An air bag has a fixed volume, which means that the amount of gas released has to be carefully con- trolled. A typical air bag contains approximately 130 g of NaN3 that can produce 67 L of N, gas when NaN3 decomposes. If an insufficient amount of nitrogen were produced, the air bag would under inflate and
Transcribed Image Text:Chemistry in Action Air Bags and Stoichiometry Air bags are part of the mandatory safety systems in passenger vehicles currently sold in the United States. An air bag inflates upon collision and prevents the driver or passenger from hitting the steering wheel, dash- board, or windshield. An air bag also absorbs some of the force resulting from the collision by immediately deflating through vents when the dri- ver or passenger hits the air bag Air bags are amazing devices. They must inflate within 0.04 seconds of a collision. Because a collision cannot not provide adequate protection. Clearly, the stoichiometry of the reaction is very important. The safety of the chemical products produced in air bags is also an impor- reactive to be considered safe. A third ingredient, silicon dioxide, SiO2, the main ingredient in sand, reacts with the sodium oxide and potassium oxide to form a safe, stable silicate glass. As a result, all of the harmful products generated during the air bag inflation are converted into safe substances. tant consideration. Sodium azide is highly toxic, but it is entirely con- sumed in the decomposition reaction. The sodium that is produced by the sodium azide decomposition can react explosively with water to produce sodium hydroxide and hydrogen. Potassium nitrate, KNO, is mixed with the sodium azide because KNO3 can react with the sodium metal to pro- duce safer compounds, as shown in the following unbalanced equation: However, the reaction of the potassi- um nitrate with the sodium metal also produces nitrogen gas, which will increase the volume of gas inside the air bag. Careful stoichiometric calcula- tions are needed to choose the correct amount of reactants to yield the total volume of nitrogen required for the air bag to function properly. be predicted, the inflation system must be ready to activate at any time during the life of the vehicle. The rapid chemical decomposition of solid sodi- um azide, NaN, allows the air bag to inflate fast at any time. The decompo- sition reaction is initiated in a car by a small ignition induced by a collision sensing mechanism. The nitrogen gas produced during the reaction inflates the air bag. Although NaN, is stable at room temperature, it decomposes into solid sodium and nitrogen gas at tem- peratures above 300°C by the reac- tion shown beloW. KNO,(s) + Na(s)→ Question 1. Balance the equation for the reaction of potassium nitrate K,0(s) + Na,0(s) + N2(g) Another chemical reaction is still required because the potassium oxide, K,0, and sodium oxide, Na,O, are too and sodium. V An air bag inflates with nitrogen in 0.04 seconds. 2NAN3(s) → 2Na(s) + 3N,(g) An air bag has a fixed volume, which means that the amount of gas released has to be carefully con- trolled. A typical air bag contains approximately 130 g of NaN3 that can produce 67 L of N, gas when NaN3 decomposes. If an insufficient amount of nitrogen were produced, the air bag would under inflate and
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