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

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asked by Robert
  1. This will get you to mm Hg, then divide mm by 760 mm to change to atm.

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