# Question f7f3a

Jun 19, 2017

${\text{N"_2(g) + 3"H"_2(g) rightleftharpoons 2"NH}}_{3} \left(g\right)$

#### Explanation:

The Haber process is arguably one of the most important chemical processes in the industrial world. In the process, nitrogen gas and hydrogen gas combine to form ammonia:

${\text{N"_2(g) + "H"_2(g) rightleftharpoons "NH}}_{3} \left(g\right)$ (unbalanced)

To balance this equation, let's start by placing a coefficient of color(red)(2 in front of ${\text{NH}}_{3}$ to balance the nitrogen:

${\text{N"_2(g) + "H"_2(g) rightleftharpoons color(red)(2)"NH}}_{3} \left(g\right)$ (unbalanced)

Now we notice there are $6$ hydrogens on the right and $2$ on the left. To fix this, we simply place a color(blue)(3# in front of the ${\text{H}}_{2}$:

${\text{N"_2(g) + color(blue)(3)"H"_2(g) rightleftharpoons color(red)(2)"NH}}_{3} \left(g\right)$ (balanced)

And our equation is balanced:)