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pentagon [3]
3 years ago
11

How many grams of nan3 are required to produce 19.0 ft3 of nitrogen gas, about the size of an automotive air bag, if the gas has

a density of 1.25 g/l?
Chemistry
1 answer:
Papessa [141]3 years ago
3 0

The  balanced chemical reaction is given as:

2NaN_{3}(s)\rightarrow 2Na(s)+3N_{2}(g)

Now, convert 19.0 ft^{3} into litres.

1 ft^{3}  = 28.3168

So, 19.0 ft^{3} = 19\times 28.3168 = 538.0192 L

Density is equal to the ratio of mass to the volume.

D=\frac{M}{V}

where, M = mass and V= volume (538.0192 L)

Substitute the value of density and volume in formula to get the value of mass.

1.25 g/L=\frac{M}{538.0192 L}

1.25 g/L\times 538.0192 L= M

Mass = 672.524 g

Now, number of moles of N_{2} gas=\frac{672.524 g}{28.02 g/mol}

= 24.00 moles

According to the reaction, 2 moles of sodium azide gives 3 moles of nitrogen gas.

Now, in 24.00 moles of nitrogen gas produced from= \frac{2 moles of sodium azide}{3 moles of nitrogen gas}\times 24.00 moles of nitrogen gas, moles of sodium azide.

number of moles of sodium azide  = 16 moles

Mass of sodium azide in g  =  number of moles\times molar mass of sodium azide.

= 16 moles\times 65.00 g/mol

= 1040 g

Thus, mass of sodium azide which is required to produce 19.0 ft^{3} of nitrogen gas  = 1040 g





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