Posted by **JamieLyn** on Tuesday, May 25, 2010 at 12:30pm.

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? It seems to be alot of liters!

Thank you

## Answer This Question

## Related Questions

- Chemistry-Could you check this, please? - I have a balloon that contains 22 ...
- Chemistry - I forgot in my previous question to say 1014 millibars. The question...
- Chemistry - I live in an area of 1014 millibars barometric pressure and I have ...
- Chemistry - Help-I'm really confused-The barometric pressure in my area is 1014 ...
- chemistry - Given a balloon you have at home, to determine the barometric ...
- Chemistry - I have to chane the barometric pressure in my area to ATM. We have ...
- chem - well it saids: A 1.50L rubber balloon is filled with carbon dioxide gas ...
- Chemistry - A piece of dry ice (solid carbon dioxide) with a mass of 30.5g is ...
- Chemistry - A balloon filled with 1.35 atm of dimethyl ether gas and 5.25 atm of...
- Chemistry - A piece of dry ice (solid carbon dioxide) with a mass of 25.5 g is ...

More Related Questions