How do you calculate the volume of 89.09 grams of chlorine gas at STP?

1 Answer
anor277
May 26, 2018

Well, you define #"STP"# first....I get approx. #30*L#

Explanation:

According to the site, #"STP"# specifies a temperature of #273.15*K#, and a pressure of #100*kPa#...

And so we solve the Ideal Gas equation with the appropriate gas constant...

#V=(nRT)/P=((89.09*g)/(70.90*g*mol^-1)xx8.314*(L*kPa)/(K*mol)xx273.15*K)/(100*kPa)#

#-=??*L#

I got the gas constant from this from this site. Most chemists of my generation would habitually use #R=0.0821*(L*atm)/(K*mol)# but that ain't good enuff for IUPAC... Fortunately, the Gas constants, and the appropriate units, would appear as supplementary material in an examination.

Note that you must simply KNOW that chlorine is a bimolecular gas, i.e. #Cl_2#.. In fact most of the elemental gases, hydrogen, oxygen, chlorine, fluorine, certainly the ones with any chemistry, are bimolecular species...

Related questions
See all questions in Gas Pressure
Impact of this question
3966 views around the world
You can reuse this answer
Creative Commons License