Based on the stoichiometry of the reaction, If the mass of sodium azide used was far greater than 1424 g, the volume of nitrogen gas produced will be far greater than 736 L.
However, If the mass of sodium azide used was far less than 1424 g, the volume of nitrogen gas produced will be far less than 736 L.
Sodium azide is the chemical found in automobile airbags.
Automotive air bags inflate when an electrical charge triggered by automobile impact causes sodium azide, NaN3, to rapidly decompose to its component elements, nitrogen gas and sodium
The equation of the reaction is given below:
According to the equation of reaction, 2 moles of sodium azide produces 3 moles of nitrogen gas.
1 mole of Nitrogen gas has a volume of 22.4 L
Molar mass of sodium azide is 65 g
Moles of sodium azide in 1424 g = 1424/65 = 21.9077 moles
21.9077 moles of sodium azide will produce 21.9077 * 3/2 moles of nitrogen gas = 32.86 moles of nitrogen gas
32.86 moles of nitrogen gas will occupy a volume of 32.86 * 22.4 = 736 L
If the mass of sodium azide used was far greater than 1424 g, the volume of nitrogen gas produced will be far greater than 736 L.
If the mass of sodium azide used was far less than 1424 g, the volume of nitrogen gas produced will be far less than 736 L.
Learn more about gas volume at: https://brainly.com/question/25736513
