What mass, in grams, of chlorine gas (Cl2) is contained in a 15.5 liter tank at 25.5 degrees Celsius and 1.98 atmospheres? Show all of the work used to solve this problem.

Question

anonymous · Answer

So far I have
PV=nRT
(1.98)(15.5)= n(0.0821)(25.5)
30.69=n(2.09355)
14.65931 = n

moles=grams/molecular mass
grams = moles x mol mass
g = 14.659 x 35.453
g =

anonymous · Answer

I just want to make sure it's right

accessdenied · Answer

Your temperature was given in degrees Celsius.  But the Ideal Gas Law requires the absolute temperature in Kelvin, correct?

accessdenied · Answer

Also, the molecular mass of a single chlorine atom is 35.453 g/mol, but the question specifically uses diatomic chlorine gas (Cl_2).  You have two chlorine atoms, so you should use twice that molar mass for a unit of chlorine gas.
Other than that, the remaining steps look great.  Just some little things that are easy to overlook!