Question #7f3c3

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Aug 20, 2017

Answer:

#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"#.

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