What mass of nitride can be obtained by reacting 22 liters of nitrogen with lithium if the mass

What mass of nitride can be obtained by reacting 22 liters of nitrogen with lithium if the mass fraction of the yield is 90%?

Based on the data, we write down the process equation:
N2 + 6Li = 2Li3N – compounds, lithium nitride is released;

Calculations:
M (Li3N) = 34.7 g / mol.

Proportions:
1 mole of gas at normal level – 22.4 liters;

X mol (N2) -22 L hence, X mol (N2) = 1 * 22 / 22.4 = 0.98 mol;

0.98 mol (N2) – X mol (Li3N);

-1 mol -2 mol hence, X mol (Li3N) = 0.98 * 2/1 = 1.96 mol.

We find the mass of nitride taking into account the product yield:
m (Li3N) = Y * M = 1.96 * 34.7 = 68.01 g (theoretical weight);

m (Li3N) = 0.90 * 68.01 = 61.2 g (practical weight).

Answer: Received lithium nitride weighing 61.2 g