Chemistry
posted by Robert .
I forgot in my previous question to say 1014 millibars. The question is I live at 1014 millibars for barometric pressure and temp. is 61 degrees Fahrenheit. I have an imaginary balloon that contains 22 grams of CO2what is the volume in liters of the balloon using the gas constant. I know I use the ideal gas law but how do I change the barometric pressure from millibars to atm

This will get you to mm Hg, then divide mm by 760 mm to change to atm.
http://www.google.com/search?q=1+bar+to+mm+Hg&ie=utf8&oe=utf8&aq=t&rls=org.mozilla:enUS:official&client=firefoxa
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