I am doing multiple ungraded practices on airbags for an upcoming quiz. This is one of the practices i have found online. Read the article i have attached and then answer the questions. Thank you :) 1. What type of reaction occurs initially with sodium azide when airbags initially deploy?2. Write the complete, balanced reaction below.3. What would happen if the manufacturers did not start with the correct amount of sodium azide?4. Based on the article, what is stoichiometry? Why is it important for airbag safety?5. Why is potassium nitrate also in airbags? 6. Write the balanced equation for the reaction between potassium nitrate and sodium below.7. What is the point of silicon dioxide?8. Why are careful stoichiometric calculations important for air bags and safety Chemistry in ActionAir Bags and StoichiometryAir bags are part of the mandatorysafety systems in passenger vehiclescurrently sold in the United States. Anair bag inflates upon collision andprevents the driver or passenger fromhitting the steering wheel, dash-board, or windshield. An air bag alsoabsorbs some of the force resultingfrom the collision by immediatelydeflating through vents when the dri-ver or passenger hits the air bagAir bags are amazing devices. Theymust inflate within 0.04 seconds of acollision. Because a collision cannotnot provide adequate protection.Clearly, the stoichiometry of thereaction is very important.The safety of the chemical productsproduced in air bags is also an impor-reactive to be considered safe. A thirdingredient, silicon dioxide, SiO2, themain ingredient in sand, reacts withthe sodium oxide and potassium oxideto form a safe, stable silicate glass. Asa result, all of the harmful productsgenerated during the air bag inflationare converted into safe substances.tant consideration. Sodium azide ishighly toxic, but it is entirely con-sumed in the decomposition reaction.The sodium that is produced by thesodium azide decomposition can reactexplosively with water to producesodium hydroxide and hydrogen.Potassium nitrate, KNO, is mixed withthe sodium azide because KNO3 canreact with the sodium metal to pro-duce safer compounds, as shown inthe following unbalanced equation:However, the reaction of the potassi-um nitrate with the sodium metal alsoproduces nitrogen gas, which willincrease the volume of gas inside theair bag. Careful stoichiometric calcula-tions are needed to choose the correctamount of reactants to yield the totalvolume of nitrogen required for the airbag to function properly.be predicted, the inflation systemmust be ready to activate at any timeduring the life of the vehicle. The rapidchemical decomposition of solid sodi-um azide, NaN, allows the air bag toinflate fast at any time. The decompo-sition reaction is initiated in a car by asmall ignition induced by a collisionsensing mechanism. The nitrogen gasproduced during the reaction inflatesthe air bag. Although NaN, is stable atroom temperature, it decomposes intosolid sodium and nitrogen gas at tem-peratures above 300°C by the reac-tion shown beloW.KNO,(s) + Na(s)→Question1. Balance the equation for thereaction of potassium nitrateK,0(s) + Na,0(s) + N2(g)Another chemical reaction is stillrequired because the potassium oxide,K,0, and sodium oxide, Na,O, are tooand 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 gasreleased has to be carefully con-trolled. A typical air bag containsapproximately 130 g of NaN3 thatcan produce 67 L of N, gas whenNaN3 decomposes. If an insufficientamount of nitrogen were produced,the air bag would under inflate and

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Answered: I am doing multiple ungraded practices…

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter5: Gases

Section: Chapter Questions

Problem 130E