posted by JamieLyn on .
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!
Remember at STP one mole is 22.4 liters, you have one half mole, at near STP. Your answer is reasonalbe.