A2.95 g sample of an unknown chlorofluorocarbon (an organic compound containing chlorine and fluorine) is decomposed and produces 581 ml of chlorine gas at a pressure of 752 mmhg and a temperature of 298 k. what is the percent by mass of chlorine in the chlorofluorocarbon?

mass percent of chlorine is 56.5%

Explanation:

Given data:

Volume V = 581 mL = 0.581 L

Pressure P = 752 mm of Hg = 752/760 = 0.9894 atm

Temperature T = 298 K

Molar gas constant R = 0.08206 atm.L/mol.K

from Ideal gas equation we have following relation

PV = nRT solving for n

n = 0.0235 mole

mas of  = moles × molar mass of

Mass percent of chlorine  

a lot of it means it can be "burned" for energy and sold at one price. if it is scarce, the price will go up

grav potential energy