   # Sodium azide, the explosive compound in automobile air bags, decomposes according to the following equation: 2 NaN 2 (s) → 2 Na(s) + 3 N 2 (g) What mass of sodium azide is required to provide the nitrogen needed to inflate a 75.0-L bag to a pressure of 1.3 atm at 25 °C? ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 10, Problem 33PS
Textbook Problem
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## Sodium azide, the explosive compound in automobile air bags, decomposes according to the following equation:2 NaN2(s) → 2 Na(s) + 3 N2(g)What mass of sodium azide is required to provide the nitrogen needed to inflate a 75.0-L bag to a pressure of 1.3 atm at 25 °C?

Interpretation Introduction

Interpretation:

The mass of sodium azide required has to be calculated.

Concept Introduction:

According to ideal gas equation:

PV=nRT

Numberofmoles=massmolarmass

### Explanation of Solution

Given that:

Pressure=1.3atmVolume=75LTemperature=25°C=298K

According to ideal gas equation:

PV=nRT

n=PVRT=1.3atm×75L0.08205L.atm/K.mol×298K=3.99molN2

Now we have to calculate the quantity of NaN2 that will produce 3

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