Question

Question #f7f3a

Answer 1

`"N"_2(g) + 3"H"_2(g) rightleftharpoons 2"NH"_3(g)`

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:

`"N"_2(g) + "H"_2(g) rightleftharpoons "NH"_3(g)` (unbalanced)

To balance this equation, let's start by placing a coefficient of `color(red)(2` in front of `"NH"_3` to balance the nitrogen:

`"N"_2(g) + "H"_2(g) rightleftharpoons color(red)(2)"NH"_3(g)` (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 `"H"_2`:

`"N"_2(g) + color(blue)(3)"H"_2(g) rightleftharpoons color(red)(2)"NH"_3(g)` (balanced)

And our equation is balanced:)