# Determine how many liters of nitrogen will be required to produce 214.4 liters of ammonia? The balanced equation for this reaction is: 3"H"_2(g) + "N"_2(g) -> 2"NH"_3(g) ?

Dec 21, 2017

$\text{107.2 L}$

#### Explanation:

The idea here is that if all the gases that take part in the reaction are kept under the same conditions for pressure and temperature, then you can treat the mole ratios that exist between them as volume ratios.

$3 {\text{H"_ (2(g)) + "N"_ (2(g)) -> 2"NH}}_{3 \left(g\right)}$

The balanced chemical equation tells you that in order to produce $2$ moles of ammonia, the reaction must consume $3$ moles of hydrogen gas and $1$ mole of nitrogen gas.

If all three gases are kept under the same conditions for pressure and temperature, you can say that in order for the reaction to produce $\text{2 L}$ of ammonia, ti must consume $\text{3 L}$ of hydrogen gas and $\text{1 L}$ of nitrogen gas.

This means that your reaction will require

$214.4 \textcolor{red}{\cancel{\textcolor{b l a c k}{{\text{L NH"_3))) * "1 L N"_2/(2color(red)(cancel(color(black)("L NH"_3)))) = color(darkgreen)(ul(color(black)("107.2 L N}}_{2}}}}$

The answer is rounded to four sig figs.