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…

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter18: Chemical Equilibrium

Section: Chapter Questions

Problem 83E

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Similar questions

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A 4.72-g sample of methanol (CH3OH) was placed in an otherwise empty 1.00-L flask and heated to 250.C to vaporize the methanol. Over time, the methanol vapor decomposed by the following reaction: CH3OH(g)CO(g)+2H2(g) After the system has reached equilibrium, a tiny hole is drilled in the side of the flask allowing gaseous compounds to effuse out of the flask. Measurements of the effusing gas show that it contains 33.0 times as much H2(g) as CH3OH(g). Calculate K for this reaction at 250.C.
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A gaseous material XY(g) dissociates to some extent to produce X(g) and Y(g): XY(g)X(g)+Y(g) A 2.00-g sample of XY (molar mass = 165 g/mol) is placed in a container with a movable piston at 25C. The pressure is held constant at 0.967 atm. As XY begins to dissociate, the piston moves until 35.0 mole percent of the original XY has dissociated and then remains at a constant position. Assuming ideal behavior, calculate the density of the gas in the container after the piston has stopped moving, and determine the value of K for this reaction of 25C.

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