Question

Question #7f3c3

Answer 1

`69.2` `"L N"_2`

Explanation:

We're asked to find the volume (in liters) occupied by `86.5` `"g N"_2`.

I'll assume the conditions are standard temperature and pressure.

If these conditions are `1` `"atm"` and `273.15` `"K"` (`0` `""^"o""C"`), then one mole of an (ideal) gas occupies a volume of `22.4` `"L"`.

With that in mind, let's first convert from grams of nitrogen to moles, using its molar mass:

`86.5cancel("g N"_2)((1color(white)(l)"mol N"_2)/(28.013cancel("g N"_2))) = color(red)(ul(3.09color(white)(l)"mol N"_2`

Now, we use the above conversion factor

`ul(1color(white)(l)"mol" = 22.4color(white)(l)"L"`

to convert from moles to liters:

`color(red)(3.09)cancel(color(red)("mol N"_2))((22.4color(white)(l)"L N"_2)/(1cancel("mol N"_2))) = color(blue)(ulbar(|stackrel(" ")(" "69.2color(white)(l)"L N"_2" ")|)`

Therefore, `86.5` grams of nitrogen occupies a volume of `color(blue)(69.2color(white)(l)"liters"`.