To determine how many moles of lithium nitride (Li₃N) would be produced from 12 moles of lithium (Li) reacting with excess nitrogen, we can use the balanced chemical equation:
\[ 6Li + N_2 → 2Li_3N \]
From the equation, we can see that:
- 6 moles of lithium produce 2 moles of lithium nitride.
Now, to find out how much lithium nitride is produced from 12 moles of lithium, we can set up a ratio based on the coefficients from the balanced equation:
\[ \text{If } 6 \text{ moles of Li produce } 2 \text{ moles of Li}_3N: \]
\[ 12 \text{ moles of Li will produce } x \text{ moles of Li}_3N. \]
Using the ratio:
\[ \frac{2 \text{ moles of Li}_3N}{6 \text{ moles of Li}} = \frac{x \text{ moles of Li}_3N}{12 \text{ moles of Li}} \]
Cross-multiplying gives:
\[ x \cdot 6 = 2 \cdot 12 \]
\[ 6x = 24 \]
Dividing both sides by 6:
\[ x = 4 \]
So, 12 moles of lithium will produce 4.0 moles of lithium nitride.
The correct answer is: A. 4.0 mol.
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