Posted by **JamieLyn** on Monday, May 24, 2010 at 4:32pm.

I have a balloon that contains 22 grams of Carbon dioxide. The barometric pressure is 1019 millibars which I converted to 1.006 Atm and the temperature is 299 "K". What is the volume of balloon? I used the ideal gas law to find out the volume in liters of the balloon.

Is my calculation correct?

1.006 Atm times unknown Volume = 0.5 Moles of CO2 times 0.0821 times 299

1.006 Atm times Volume = 12.27

I then took 12.27/1.006 and came up with 12.2 L of the balloon. Is this correct? If not where did I go wrong?

Thank you

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