Question

What mass in grams of NaN₃ is required to produce 50.2 L of N₂ gas (density = 1.25 g/L) according to the balanced chemical reaction: 2NaN₃(s) > 2Na(s) + 3N₂(g)

Answer 1

To find the mass of NaN3 needed to produce 50.2 L of N2 gas, multiply the volume by the density to get the mass of N2, convert this to moles using its molar mass, then use the stoichiometry of the balanced reaction, and finally, multiply by the molar mass of NaN3 to get the required mass.

Step-by-step explanation:

The student asked about the mass of sodium azide (NaN3) required to produce 50.2 L of nitrogen (N2) gas, given the balanced reaction 2NaN3(s) → 2Na(s) + 3N2(g). First, calculate the mass of N2 by multiplying the volume (50.2 L) by the density (1.25 g/L), which equals 62.75 g. Next, use the molar mass of N2 (28.02 g/mol) to find the moles of N2, and then use the stoichiometry of the reaction to calculate the moles of NaN3 required. Lastly, multiply by the molar mass of NaN3 (65.01 g/mol) to find the required mass of NaN3.