Air bags in cars are inflated by the sudden
decomposition of sodium azide (NaN3) by the
following reaction.
2 NaN3(s) −→ 3 N2(g) + 2 Na(s)
What volume of N2 gas, measured at 1.31
atm and 85.0◦C, would be produced by the
reaction of 65.0 g of NaN3?
Answer in units of L
Refer to your post just below. Same process. Post your work if you get stuck and tell us what you don't understand. We can help you through it..
To find the volume of N2 gas produced, we need to use the ideal gas law equation:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in L)
n = number of moles
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature (in Kelvin)
First, we need to calculate the number of moles of N2 gas produced. To do this, we can use the molar mass of NaN3.
1 mole of NaN3 = 65.0 g (given)
Convert grams of NaN3 to moles of NaN3 by dividing the given mass by the molar mass:
moles of NaN3 = 65.0 g / molar mass of NaN3
Molar mass of NaN3 = (1 Na x atomic mass of Na) + (3 N x atomic mass of N)
= (1 x 22.99 g/mol) + (3 x 14.01 g/mol)
= 22.99 g/mol + 42.03 g/mol
= 65.02 g/mol
moles of NaN3 = 65.0 g / 65.02 g/mol
Now, we can use the stoichiometry of the reaction to find the number of moles of N2 gas produced:
From the balanced equation:
2 NaN3(s) → 3 N2(g) + 2 Na(s)
The mole ratio is:
2 moles of NaN3 : 3 moles of N2
moles of N2 = (moles of NaN3) x (3/2)
Substitute the value of moles of NaN3 to find moles of N2.
Next, let's convert the temperature to Kelvin:
Kelvin = Celsius + 273.15
T = 85.0°C + 273.15 = 358.15 K
Now we can substitute the values into the ideal gas law equation:
PV = nRT
V = (nRT) / P
V = [(moles of N2) x (0.0821 L·atm/mol·K) x (358.15 K)] / (1.31 atm)
Solve the equation to find the volume of N2 gas produced in liters (L). Round your answer to the appropriate number of significant figures.