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Automotive air bags inflate when a sample of sodium azide, NaN $_{3},$ is very rapidly decomposed. $2 \mathrm{NaN}_{3}(s) \longrightarrow 2 \mathrm{Na}(s)+3 \mathrm{N}_{2}(g)$What mass of sodium azide is required to produce 2.6 $\mathrm{ft}^{3}(73.6 \mathrm{L})$ of nitrogen gas with a density of 1.25 $\mathrm{g} / \mathrm{L} ?$
142 $\mathrm{g} \mathrm{NaN}_{3}$
00:46
Sisi G.
Chemistry 101
Chapter 4
Stoichiometry of Chemical Reactions
Chemical reactions and Stoichiometry
Keltoum M.
May 31, 2021
Equal numbers of moles of H2(g), Ar(g), and N2(g) are placed in a glass vessel at room temperature. If the vessel has a pinhole-sized leak, which of the following will be true regarding the relative values of the partial pressures of the gases remaining i
Carleton College
Brown University
Lectures
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This next question is in reference to the decomposition of sodium aside, which is used to rapidly inflate the airbags in automobiles. The reaction is to sodium asides, going to to sodium and three nitrogen molecules. It wants to know the mass of sodium azide required to produce 73.6 liters of nitrogen gas. So we'll start with a 73 6 liters of nitrogen gas. The density of the nitrogen gas is provided 1.25 g per liter. This will allow us to convert the leaders nitrogen gas into grams nitrogen gas well, then divide by the molar mass of nitrogen gas to get the moles of nitrogen gas so that we can use the stock geometry of the balanced chemical reaction to get out of units nitrogen gas and into units of sodium Aside, with a 3 to 2 more relationship when we have moles sodium azide, we can multiply by the molar mass of sodium azide to get gram sodium azide so it looks like 142 g of sodium acetate are required to produce 73.6 leaders of nitrogen gas.
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