Automobile air bags employ a chemical reaction involvingthe rapid decomposition of sodium azide (NaN3) intosodium metal and nitrogen gas to inflate in a collision. Howmuch sodium azide is required to decompose to inflate a20.0 L air bag? Assume that the gas is at standardtemperature and pressure, and thus occupies 22.4 L permole. (AW: Na=23; N=14.007)...A76.3 g42.8 g38.7 g62.7 g

2NaN3 →2Na(s)+3N2(g) Molar Mass of NaN3= 65.021 g/mol Volume of gas at STP= 22.4L Standard…

Answered: Automobile air bags employ a chemical…

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter8: Gases

Section: Chapter Questions

Problem 94E: Xenon and fluorine will react to form binary compounds when a mixture of these two gases is heated...

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Similar questions

What possible uses exist for the natural gas liquids that are removed from natural gas during its processing?
Xenon and fluorine will react to form binary compounds when a mixture of these two gases is heated to 400C in a nickel reaction vessel. A 100.0-mL nickel container is filled with xenon and fluorine, giving partial pressures of 1.24 atm and 10.10 atm, respectively, at a temperature of 25C. The reaction vessel is heated to 400C to cause a reaction to occur and then cooled to a temperature at which F2 is a gas and the xenon fluoride compound produced is a nonvolatile solid. The remaining F2 gas is transferred to another 100.0-mL nickel container, where the pressure of F2 at 25C is 7.62 atm. Assuming all of the xenon has reacted, what is the formula of the product?
At elevated temperatures, sodium chlorate decomposes to produce sodium chloride and oxygen gas. A 0.8765-g sample of impure sodium chlorate was heated until the production of oxygen gas ceased. The oxygen gas collected over water occupied 57.2 mL at a temperature of 22C and a pressure of 734 torr. Calculate the mass percent of NaClO3 in the original sample. (At 22C the vapor pressure of water is 19.8 torr.)
How does hydraulic fracturing differ from previously used techniques for the recovery of natural gas from the earth?
When two cotton plugs. one moistened with ammonia and the other with hydrochloric acid, are simultaneously inserted into opposite ends of a glass tube that is 87.0 cm long, a white 1111g of NH4Cl forms where gaseous NH3 and gaseous HC1 first come into contact. NH3(g)+HCl(g)NH4Cl(s) At approximately what distance from the ammonia moistened plug does this occur? (Hint: Calculate the rates of diffusion for both NH3 and HCI, and find out how much faster NH3 diffuses than HCI.)
95 Some engineering designs call for the use of compressed air for underground work. If water containing iron(II) ions is present, oxygen in the compressed air may react according to the following unbalanced net ionic equation: Fe2++H++O2Fe3++H2O (a) Write the balanced net ionic equation. Remember that the amounts of each substance and the charges must balance. (b) Assume all of the oxygen from 650 L of compressed air at 15°C and 6.5 atm is lost by this reaction. What mass of water would be produced? (The mole fraction of oxygen in air is about 0.21.) (c) What will be the final pressure after the loss of the oxygen?
A gaseous hydrocarbon reacts completely with oxygen gas to form carbon dioxide and water vapour. Given the following data, determine Hf for the hydrocarbon: Hreaction=2044.5KJ/molhydrocarbonHf(CO2)=393.5KJ/molHf(H2O)=242KJ/mol Density of CO2 and H2O product mixture at 1.00 atm, 200.c = 0.751g/L. The density of the hydrocarbon is less than the density of Kr at the same conditions.

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