Question

13.
Automobile air bags are inflated with N2 gas which is formed by the decomposition of solid
sodium azide(NaN). The other product is Na - metal. Calculate the volume of N2 gas at 27°C
and 756 Torr formed by the decomposing of 125 gm of sodium azide

Answer 1

71.65 L of $N_2$ gas at 27°C  and 756 Torr formed by the decomposing of 125 gm of sodium azide

Explanation:

The decomposition reaction for solid sodium azide is:

$2NaN_3(s)\rightarrow 2Na(s)+3N_2(g)$

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

$\text{Number of moles of sodium azide}=\frac{125g}{65.g/mol}=1.92moles$

According to stoichiometry:

2 moles of $NaN_3$ gives = 3 moles of $N_2$

Thus 1.92 moles of $NaN_3$ will produce=$\frac{3}{2}\times 1.92=2.88$ moles of $N_2$

According to the ideal gas equation:

According to the ideal gas equation:'

$PV=nRT$

P = Pressure of the gas = 756 torr = 0.99 atm    (1 torr= 0.0013 atm)

V= Volume of the gas = ?

T= Temperature of the gas = 27°C = 300 K       (0°C = 273 K)

R= Gas constant = 0.0821 atmL/K mol

n=  moles of gas= 2.88  

$V=\frac{nRT}{P}=\frac{2.88\times 0.0821\times 300}{0.99}=71.65L$

Learn More

https://brainly.com/question/12947144

https://brainly.com/question/13274658

#learnwithbrainly