Chemistry Homeworkkkk

A sample of fluorine gas occupies 855 mL at 710 mm Hg at 155 degrees C.
a) What is the mass of the sample?
b)What is the density of fluorine at this temperature and pressure?

Please show your work and thank you so much :)

The equation to find out how much mass you have is the amount of moles, times the molar mass of fluorine gas, F2. To find the moles you have to use the PV=nRT formula, which is (pressure)(volume)=(number of moles)(gas ratio)(Kelvin temperature)
So the formula goes: (710mmHg)(.855L)=n(62.4)(428)
In the end, n=607.05/26707.2= .0227 moles
Then you take .0227mol. times 38g (molar mass of F2) Which equals .863 grams.
Then you divide that number by the number of liters, .855 to find the density, which ends up being 1.009 g/L

Calculate the moles of Fl2 using the ideal gas law PV=nRT

The mass is the moles of fluorine * the molecular weight of fluorine

Density = P * MW / (R * T)