Automobile airbags contain solid sodium azide, nan 3 , that reacts to produce nitrogen gas when heated, thus inflating the bag. 2 nan 3 ( s ) ⟶ 2 na ( s ) + 3 n 2 ( g ) calculate the value of work, w , for the system if 16.5 g nan 3 reacts completely at 1.00 atm and 22 ∘ c.

The value of work for the system is -935.23 J

Explanation:

To calculate the number of moles, we use the equation:

Given mass of sodium azide = 16.5 g

Molar mass of sodium azide = 65 g/mol

Putting values in above equation, we get:

The given chemical equation follows:

By Stoichiometry of the reaction:

2 moles of sodium azide produces 3 moles of nitrogen gas

So, 0.254 moles of sodium azide will produce = of nitrogen gas

To calculate volume of the gas given, we use the equation given by ideal gas, which follows:

where,

P = pressure of the gas = 1.00 atm

V = Volume of the gas = ?

T = Temperature of the gas =

R = Gas constant =

n = number of moles of nitrogen gas = 0.381 moles

Putting values in above equation, we get:

To calculate the work done for expansion, we use the equation:

We are given:

P = pressure of the system =     (Conversion factor:  1 atm = 101325 Pa)

= change in volume =     (Conversion factor:   )

Putting values in above equation, we get:

Hence, the value of work for the system is -935.23 J

it is a good conductor

explanation:

the correct answer would be d. hope this !