A helium filled balloon has a volume of 750L at 8*C @ pressure of 380 torr. New vol is 0.20atm & temp -45*C?

What is the new volume of the balloon?

A helium filled balloon has a volume of 750L at 8*C @ pressure of 380 torr. New vol is 0.20atm %26amp; temp -45*C?
You can use the ideal gas law to solve this problem fairly easily. Since the balloon is closed, the number of moles before and after the change is constant. So solve the ideal gas law for the number of moles and set the before equal to the after. Then solve for the volume after (V2) to get a function that is the initial volume times the ratio of before and after temperatures and pressures. Then just plug in your numbers, and make sure that your units are consistent and that you use Kelvin for temperature.





V2 = 1521 liter
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