anonymous
  • anonymous
WILL GIVE MEDALS . (: What mass, in grams, of chlorine gas (Cl) 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.
Chemistry
  • Stacey Warren - Expert brainly.com
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schrodinger
  • schrodinger
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anonymous
  • anonymous
\[n=(1.98 atm*15.5L)/(0.08206Latm*298.65K)\] There, the ideal gas equation is all set up for you to obtain the number of moles of chlorine gas. Then, you must use the molar mass of chlorine gas, Cl2 remember, to convert the moles to mass in grams.
anonymous
  • anonymous
(V)Volume = 22.41L (T)Temperature = 273K or 0.0 Celsius (P)Pressure = 1.0atm R value is always .08206 with atm n = moles V = nRP/K sub what you have into the equation
anonymous
  • anonymous
Ignore the variables as they corrospond to standard temperture and pressure

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anonymous
  • anonymous
once you have the moles its as easy as using the formula moles = grams/Molecular Mass
anonymous
  • anonymous
appy formula for ideal gas as PV=nRT

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