# What is the theoretical yield of Li_3N in grams when 12.5 g of Li ls heated with 34.1 g of N_2?

Nov 15, 2015

The theoretical yield of $\text{Li"_3"N}$ is $\text{20.9 g}$.

#### Explanation:

Balanced Equation

"6Li(s)" + "N"_2("g")$\rightarrow$$\text{2Li"_3"N(s)}$

In order to determine the theoretical yield, we must first find the limiting reactant (reagent), which will determine the greatest possible amount of product that can be produced.

Molar Masses
$\text{Li} :$$\text{6.941 g/mol}$
$\text{N"_2} :$(2xx14.007"g/mol")="28.014 g/mol"
$\text{Li"_3"N} :$(3xx6.941 "g/mol Li") + (1xx14.007"g/mol N")="34.83 g/mol Li"_3"N"

Limiting Reactant
Divide the mass of each reactant by its molar mass, then multiply times the mole ratio from the balanced equation with the product on top and the reactant on bottom, then multiply times the molar mass of $\text{Li"_3"N}$.

Lithium
$12.5 \text{g Li"xx(1"mol Li")/(6.941"g Li")xx(2"mol Li"_3"N")/(6"mol Li")xx(34.83"g Li"_3"N")/(1"mol Li"_3"N")="20.9 g Li"_3"N}$

Nitrogen Gas
$34.1 \text{g N"_2xx(1"mol N"_2)/(28.014"g N"_2)xx(2"mol Li"_3"N")/(1"mol N"_2)xx(34.83"g Li"_3"N")/(1"mol Li"_3"N")="84.8 g Li"_3"N}$

Lithium produces less lithium nitride than nitrogen gas. Therefore, the limiting reactant is lithium, and the theoretical yield of lithium nitride is $\text{20.9 g}$.