How many grams of Si3N4 can be produced from 0.46 moles of N2?

Question

3 Si + 2 N2 → Si3N4

Answer 1

Hi Diego! The work for this problem would look something like this:

0.46 mol N₂ x 1 mol Si₃N₄ x 140.31 g Si₃N₄ = 32.27g Si₃N₄ (32 g with 2 sig figs)

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2 mol N₂ 1 mol Si₃N₄

So the final answer would be 32.27 g of Si₃N₄ produced (32 g if you need to take into account sig figs). Hope this helps! Feel free to reach out with additional questions.

Answer 2

First you want to multiply by the mole ratio from the balanced equation to convert over to moles of silicon nitride:

0.46 moles N₂ x 1 mole Si₃N₄ / 2 moles N₂ = 0.23 moles Si₃N₄

from there then you can convert that value over into moles by multiplying by the molar mass

0.23 moles x 140.31 g/mol = 32.27 g

so you can produce 32 grams of Si₃N₄ from 0.46 moles of N₂