# Octane (C8H18, 114.23 g/mol). The density of octane vapour 125.0 Celsius and 720.0 torr is ? and what would be the volume be if it was 2.00 moles ?

##### 1 Answer

To determine the density of octane vapor at that temperature and pressure you basically have to use the ideal gas law equation,

Notice that this form,

So, the number of moles of a substance is defined as the ratio between mass and molar mass, which means that

If you rearrange this to isolate the unknown mass and volume on one side, you'll get

Since density is defined as mass per unit of volume, the above equation will become

Plug all your values into this equation (*do not* forget to use atm and Kelvin)

**SIDE NOTE** *Vapor density is usually given in relation to the vapor density of air at those same values for temperature and pressure. You can determine the vapor density of air at 125 Celsius and 720 torr by using its molar mass, 28.97 g/mol, in the above equation.*

*You'll get 0.8406 g/L as the vapor density of air, which will make the vapor density of octane - in this context called specific gravity - equal to*

*UNITLESS*

To determine the volume use the classic-form

This time, the answer is rounded to three sig figs because of the number of sig figs in 2.00.