Use the ideal gas law to find the moles of chlorine gas Cl2 :
n=PV/RT
then, change the moles to mass using the mole mass of Cl2
finally, percentCl is mass/2.80g
A 2.80 -g sample of an unknown chlorofluorocarbon is decomposed and produces 557mL of chlorine gas at a pressure of 750mm Hg and a temperature of 298K .
What is the percent chlorine (by mass) in the unknown chlorofluorocarbon?
1 answer