# Problem: Lithium reacts with nitrogen gas according to the following reaction: 6Li(s) + N2(g) → 2Li3N(s)6 m Li(s) +   N_2 (g) ightarrow 2 m Li_3N(s)What mass of lithium is required to react completely with 57.6 mL of N2 gas at STP?

###### FREE Expert Solution

Reaction:  6Li(s) + N2(g) → 2Li3N(s)

Get mol N2:

$\overline{){\mathbf{PV}}{\mathbf{=}}{\mathbf{nRT}}}\phantom{\rule{0ex}{0ex}}\phantom{\rule{0ex}{0ex}}\frac{\mathbf{PV}}{\mathbf{RT}}{\mathbf{=}}\frac{\mathbf{n}\overline{)\mathbf{RT}}}{\overline{)\mathbf{RT}}}\phantom{\rule{0ex}{0ex}}\phantom{\rule{0ex}{0ex}}\overline{){\mathbf{n}}{\mathbf{=}}\frac{\mathbf{PV}}{\mathbf{RT}}}$

###### Problem Details

Lithium reacts with nitrogen gas according to the following reaction: 6Li(s) + N2(g) → 2Li3N(s)

What mass of lithium is required to react completely with 57.6 mL of N2 gas at STP?

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Standard Temperature and Pressure concept. You can view video lessons to learn Standard Temperature and Pressure. Or if you need more Standard Temperature and Pressure practice, you can also practice Standard Temperature and Pressure practice problems.