Homework Help: Chemistry

Posted by Robert on Wednesday, April 21, 2010 at 9:35pm.

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 CO2-what 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

Chemistry - DrBob222, Wednesday, April 21, 2010 at 9:40pm
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=utf-8&oe=utf-8&aq=t&rls=org.mozilla:en-US:official&client=firefox-a

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