Final answer:
To determine the moles of NaN3 needed for 65 grams of N2, the molar mass of N2 is used to find the moles of N2. After finding that 2.32 moles of N2 can be produced from 65 grams, the stoichiometry of the chemical reaction shows that approximately 1.55 moles of NaN3 are required, which corresponds to about 100.75 grams of NaN3.
Step-by-step explanation:
The question is asking how many moles of NaN3 must be extracted to produce 65 grams of N2. To start solving the problem, we need to consider the chemical reaction:
2NaN3 (s) → 2Na (s) + 3N2 (g)
From the balanced equation, we see that 2 moles of NaN3 produce 3 moles of N2. First, we calculate the number of moles of N2 produced from 65 grams. Using the molar mass of N2 (28.02 g/mol), we have moles of N2 = 65 g / 28.02 g/mol ~= 2.32 mol. Since 2 moles of NaN3 produce 3 moles of N2, we need (2 moles NaN3 / 3 moles N2) x 2.32 mol N2 ≈ 1.55 moles of NaN3. Finally, we convert moles of NaN3 to grams using its molar mass (65 g/mol): 1.55 moles x 65 g/mol ≈ 100.75 g. This calculation shows that the option choices provided do not match the correct answer, indicating a potential error in the question or options.