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Chemical Properties of Boron Family

Sodium azide,...

Question

Sodium azide, the explosive chemical used in automobile airbags is made by the following reaction:
$N a N O_{3} + 3 N a N H_{2} ⟶ N a N_{3} + 3 N a O H + N H_{3}$
If you combine $15.0 g N a N O_{3}$ with $15.0 g N a N H_{2}$ , what mass of $N a N_{3}$ is produced? (Round to the nearest integer)

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Solution

The balanced chemical equation for the formation of sodium azide is as given below:
$N a N O_{3} + 3 N a N H_{2} ⟶ N a N_{3} + 3 N a O H + N H_{3}$
$15.0$ g sodium nitrate corresponds to $\frac{15.0}{85} = 0.1765 m o l e s$ .
$15.0$ g of sodamide corresponds to $\frac{15.0}{39} = 0.385 m o l e s$ .
Hence, sodamide is the limiting reagent.
$0.385$ moles of sodamide will produce $\frac{0.385}{3} = 0.128 m o l e s$ of sodium azide.
The mass of sodium azide produced will be $0.128 \times 65 = 8.3 g$ .
Hence, $8$ g of $N a N_{3}$ is produced.

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