# Question #7f3c3

##### 1 Answer

#### Answer:

#### Explanation:

We're asked to find the **volume** (in *liters*) occupied by

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

If these conditions are **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,