Ch.3 - Chemical ReactionsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Automotive air bags inflate when a sample of sodium azide, NaN3, is very rapidly decomposed.2NaN3(s) ⟶ 2Na(s) + 3N2(g)What mass of sodium azide is required to produce 2.6 ft3 (73.6 L) of nitrogen gas

Solution: Automotive air bags inflate when a sample of sodium azide, NaN3, is very rapidly decomposed.2NaN3(s) ⟶ 2Na(s) + 3N2(g)What mass of sodium azide is required to produce 2.6 ft3 (73.6 L) of nitrogen gas

Problem

Automotive air bags inflate when a sample of sodium azide, NaN3, is very rapidly decomposed.

2NaN3(s) ⟶ 2Na(s) + 3N2(g)

What mass of sodium azide is required to produce 2.6 ft3 (73.6 L) of nitrogen gas with a density of 1.25 g/L?

Solution
  • We can use the density and the volume provided to get the mass of N2

  • We will be using the V in L instead of ft3

  • The mass of N2 will be used to find the moles of sodium azide and eventually the mass

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