Question

Calculate the mass of sodium azide required to decompose and produce 1.86 moles of nitrogen. Refer to the periodic table to get the atomic weights.

For context, the airbag is 58 liters when fully inflated. The air pressure inside the airbag should be 4.4 psi. This pressure value is in addition to the normal atmospheric pressure of 14.7 psi, giving a total absolute pressure of 19.1 psi, which equals 1.30 atmospheres.

(Moles of Nitrogen calculated using Ideal Gas Law)

Answer 1

Answer:Therefore, there are approximately 2.38 moles of nitrogen gas inside the fully inflated airbag

Step-by-step explanation:

To calculate the number of moles of nitrogen gas inside the fully inflated airbag, we can use the Ideal Gas Law:

PV = nRT

where P is the absolute pressure of the gas (in atmospheres), V is the volume of the gas (in liters), n is the number of moles of gas, R is the universal gas constant (0.08206 L atm/mol K), and T is the temperature of the gas (in Kelvin).

We know that the volume of the airbag is 58 liters and the absolute pressure is 1.30 atmospheres (which includes the atmospheric pressure of 1 atmosphere). We also know that the temperature inside the airbag is likely to be close to the ambient temperature, which we can assume is around 25°C or 298 K.

So, we can rearrange the Ideal Gas Law to solve for n:

n = PV/RT

n = (1.30 atm * 58 L) / (0.08206 L atm/mol K * 298 K)

n = 2.38 moles

Therefore, there are approximately 2.38 moles of nitrogen gas inside the fully inflated airbag.