Calculate the volume of nitrogen gas that will be produced in the air bag of a car when 88,8g of sodium azide is thermally decomposed at 22 C to give the bag a pressure of 1,10 atm

2NaN3 ==> 2Na + 3N2

mols NaN3 = 88.8g/molar mass NaN3 = approx 88.8/65 = about 1.4 but that's an estimate.

mols N2 produced = 1.4 mols NaN3 x (3 mols N2/2 mols NaN3) = 1.4 x 3/2) = estimated 2.
Substitute n (2) into PV = nRT at the conditions listed and solve for V in liters. Remember T must be in kelvin.

34 litres

To calculate the volume of nitrogen gas produced, we need to use the ideal gas law equation, which is:

PV = nRT

Where:
P = pressure of the gas (in atm)
V = volume of the gas (in liters)
n = number of moles of the gas
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature of the gas (in Kelvin)

First, we need to convert the given temperature from Celsius to Kelvin:
T(K) = T(C) + 273.15
T(K) = 22 + 273.15 = 295.15 K

Next, we need to calculate the number of moles of nitrogen gas using the given mass of sodium azide. To do this, we need to convert the mass to moles using the molar mass of sodium azide.

The molar mass of sodium azide (NaN3) can be calculated by adding up the atomic masses of the individual elements.
The atomic mass of sodium (Na) is 22.99 g/mol, and the atomic mass of nitrogen (N) is 14.01 g/mol.

Molar mass of NaN3 = (1 * atomic mass of Na) + (3 * atomic mass of N)
Molar mass of NaN3 = (1 * 22.99) + (3 * 14.01)
Molar mass of NaN3 = 65.98 g/mol

Now, we can calculate the number of moles of sodium azide:
n = mass / molar mass
n = 88.8 g / 65.98 g/mol
n ≈ 1.343 mol

Next, we need to rearrange the ideal gas law equation to solve for the volume V:
V = (nRT) / P

Plugging in the values:
V = (1.343 mol * 0.0821 L·atm/(mol·K) * 295.15 K) / 1.1 atm
V ≈ 33.46 L

Therefore, the volume of nitrogen gas produced in the airbag is approximately 33.46 liters.