Question

Air bags in cars inflate when an electrical spark activates sodium azide (NaN3) so that it decomposes to sodium metal, Na, and nitrogen gas, N2. In the balanced reaction equation, how many moles of nitrogen gas are formed for one mole of sodium azide? (HINT: Write the balanced chemical equation and use the molar ratio.)

Answer 1

In the decomposition of sodium azide (NaN3) used in airbags, 1.5 moles of nitrogen gas (N2) are formed for every one mole of NaN3, according to the balanced chemical equation 2 NaN3 (s) → 3 N2(g) + 2 Na (s).

Step-by-step explanation:

In the context of chemistry in everyday life, airbags in automobiles utilize a rapid chemical reaction for deployment. One commonly used chemical reaction involves the decomposition of sodium azide, NaN3. Upon collision detection in a vehicle, an electrical spark initiates this chemical reaction.

When writing the balanced chemical equation for the decomposition of sodium azide, it is shown as:

2 NaN3 (s) → 3 N₂(g) + 2 Na (s)

According to the balanced equation, three moles of nitrogen gas, N₂, are formed for every two moles of sodium azide, NaN3. Therefore, for one mole of sodium azide, 1.5 moles of nitrogen gas are produced. This stoichiometric ratio is critical in determining the correct amount of sodium azide needed for airbag inflation.